home

Physical Chemistry Edexcel Igcse - Statistics

Jump to: Answer Stats | Score Distribution | Your Scores
General Stats
  • This quiz has been taken 8 times
    7 since last reset
  • The average score is 2 of 50
Answer Stats
Hint Answer % Correct
if backward direction is exothermic what is the forward direction endothermic
50%
state the equation for moles moles = mass/Mr
50%
what does ⇌ mean reversible reaction
50%
in an exothermic reaction, is △H negative or positive negative
40%
if a reversible reaction is exothermic one way what will the other way be endothermic
33%
in an endothermic reaction, is △H negative or positive positive
33%
what colour is anhydrous copper (ii) sulfate powder white
33%
if a reversible reaction is endothermic one way what will the other way be exothermic
25%
is the dehydration of copper (ii) sulfate exothermic no
25%
what colour is ammonium chloride powder white
25%
what colour are hydrated copper (ii) sulfate crystals blue
20%
what are marble chips made of calcium carbonate
20%
is breaking bonds endothermic or exothermic endothermic
20%
99999999999999999999 describe how to carry out experiment between sodium thiosulfate and hydrochloric acid 1: draw a large cross onto a piece of paper2: place a conical flask onto the cross 3: pour sodium thiosulfate and hydrochloric acid into the beaker 4: observe the reaction directly above the flask 5: record the time taken for the cross to vanish 6: the cross vanishes because the yellow sulfur precipitate is formed
0%
what is x⁻¹ the same as 1/x
0%
what is room temp. (don't use kelvin) 20°C
0%
what is water's c 4.2 J/g °C
0%
what one thing do reactions need to take place activation energy
0%
what will happen if you carry out the calcium carbonate and hydrochloric acid experiment but with an increased temperature all the mass and volumes stay the same, just the temperature increases. The rate of reaction is much quicker than before, happens faster and reaches the end of the reaction very quickly, so it plateaus faster.
0%
state the word equation in the thermal decomposition of ammonium chloride ammonium chloride ⇌ nitrogen + hydrogen chloride
0%
what does ventilated mean an area that's air is well circulated
0%
what is a catalyst a substance that increases the rate of reaction without getting chemically changed in the process, so it isn't used up and can be used again as a catalyst.
0%
what do you use to calculate the △H average bond energies
0%
why is a dynamic equilibrium considered dynamic because the forward and backwards directions are still moving but just at the same rate
0%
9999999999999999999 what does the activation energy do breaks bonds so new bonds can be made
0%
how do we measure the rate of reaction between the decomposition of hydrogen peroxide by measuring the oxygen produced at regular intervals using a gas syringe, both sets of results (ones with and without catalyst) are plotted onto a graph
0%
how can something gain energy if the conservation of energy is true? by transferring it
0%
state the word equation between calcium carbonate and Hydrochloric acid in alphabetical order calcium carbonate + hydrochloric acid ─> calcium chloride + water + carbon dioxide
0%
what type of calcium carbonate should you use to get the fastest rate of reaction calcium carbonate powder
0%
what 5 things would you increase to increase the rate of reaction, in ascending alphabetical order catalyst, concentration of a liquid, pressure of gas, surface area of solid, temperature.
0%
9999999999999999999 what is the enthalpy change change in heat during a reaction at constant pressure
0%
state the chemical equation between ethanol and oxygen C₂H₅OH + 3O₂ ─> 2CO₂ + 3H₂O
0%
in what environment will a reversible reaction always reach dynamic equilibrium closed system
0%
in what scenario can a dynamic equilibrium take place and why closed system so no substances can escape
0%
what is the unit g the same as cm³
0%
what colour is hydrochloric acid solution colourless
0%
what colour is sodium thiosulfate solution colourless
0%
in what reaction do reactants have less energy than products endothermic reaction
0%
what does the energy released by the forward direction equal energy absorbed by the backward direction
0%
if energy is released by the forward direction then what is the backwards direction energy is absorbed
0%
what is conservation of energy energy isn't created or destroyed in a chemical reaction
0%
if energy is absorbed by the backward direction what is the forward direction energy is released
0%
what diagram can △H be represented on? energy level diagram
0%
what is a reaction profile a.k.a energy level or energy profile
0%
9999999999999999999 how do you calculate △H using bond energies Energy needed to break bonds - Energy released when forming bonds
0%
what is Q energy transferred
0%
what is the molar enthalpy change enthalpy change per mole of a substance
0%
if forward direction is endothermic what is the backwards direction exothermic
0%
is forming bonds endothermic or exothermic exothermic
0%
in what reaction do reactants have more energy than products exothermic reaction
0%
how do we see what catalysts are the best at decomposing hydrogen peroxide experiment with different catalysts
0%
describe the neutralisation experiment using a polystyrene cup with magnesium and copper (ii) sulfate First, 50cm³ of copper (II) sulfate is measured and placed into a polystyrene cupSecondly, the initial temperature of the copper (II) sulfate solution is measured and recorded. Thirdly, Magnesium is added and the maximum temperature is measured and recorded Finally, the temperature rise is calculated We use a polystyrene cup because it is an insulator and our reaction is exothermic so this cup will keep all the heat inside and not let loads escape, so it reduces heat loss. This experiment covers neutralisation, displacement and dissolving a salt.
0%
how does the position of equilibrium change when there's a decrease in pressure of this reaction: CO₍₉₎ + 2H₂ ₍₉₎ ⇌ CH₃OH₍₉₎ first, see what side has more molecules of gas. 1 molecule on right and 3 molecules on left. So if pressure decreases, position of equilibrium shifts to the left. This is because a decrease in pressure means there is more space for particles, so if we produce more molecules then we can increase the pressure so then this decrease in pressure will be balanced out by increasing pressure as more molecules per unit of volume increases pressure, so this restores equilibrium and obviously more reactant is produced because it has more gas molecules.
0%
how does the position of equilibrium change when there's an increase in pressure of this reaction: CH₄ ₍₉₎ + H₂O₍₉₎ ⇌ CO₍₉₎ + 3H₂ ₍₉₎ first, see what side has more molecules of gas. 4 molecules on right and 2 molecules on left. So if pressure increases, position of equilibrium shifts to the left. This is because an increase in pressure means there is less space for molecules, so if we produce less particles we can decrease the pressure, this cancels out the increase in pressure so equilibrium is restored and more reactant is produced because it has less gas molecules.
0%
what happens when hydrated copper (ii) sulfate is thermally decomposed forms water and anhydrous copper (ii) sulfate in an exothermic reaction
0%
999999999999999999 what is dynamic equilibrium forward and backward reactions happen at the same rate and the amounts of reactants and products stay constant
0%
what can the units of rate of reaction be g/min g/sec cm³/sec cm³/min
0%
what is the unit cm³ the same as grams
0%
9999999999999999999 describe what the graph looks like in the reaction between marble chips and hydrochloric acid graph is very steep as lot's of carbon dioxide is being produced and reaction is very fastgraph gets less steep because reaction is slowing down graph is flat as no carbon dioxide is being produced and the reaction has ended
0%
what is the difference in energy known as in a reaction profile △H
0%
what is hydrogen peroxide's chemical formula H₂O₂
0%
define the rate of reaction how quickly the products are formed or how quickly the reactants are used up
0%
state the equation for △H △H = Q/mol
0%
state the word equation for the dehydration of copper (ii) sulfate hydrated copper (ii) sulfate ⇌ anhydrous copper (ii) sulfate + water
0%
what is the symbol reversible equation for the reaction between hydrogen and nitrogen hydrogen + nitrogen ⇌ ammonia
0%
how do we know if a catalyst is effective in the decomposition of hydrogen peroxide if bubbles of oxygen gas are formed
0%
describe and explain how to increase the rate of reaction with a liquid without increasing temperature Increase the concentration of the liquid, this means more particles will be in the same volume, so there will be more particles per unit of volume, this produces more frequent collisions which increases the rate of reaction.
0%
describe and explain how to increase the rate of reaction with a gas without increasing temperature Increase the pressure of a gas, this means the same particles are present in a smaller volume which means there is less room for the gases to not react, so there are more particles per unit of volume as there is less volume for them to travel in. This makes more room for collisions so they will be more frequent which increases the rate of reaction.
0%
describe and explain how to increase the rate of reaction with a solid without increasing temperature Increase the surface area of the solid, this makes the particles more exposed meaning they are distributed further throughout the solution. This results in more frequent collisions because there are more particles spread out. This increases the rate of reaction
0%
describe and explain how to increase the rate of reaction without increasing the reactants abundance Increase the temperature of the substance, this gives the particles more kinetic energy, allowing them to move faster which means they will collide with each other more frequently. Also a higher proportion of the collisions will be successful as the collision energy will be greater than or equal to the activation energy, this means the reaction can take place more often. All of this increases the rate of reaction very well which is why increasing the temperature is one of if not the most efficient way to increase the rate of reaction.
0%
state the △H, increased temperature change, energy of products and reactants and the type of reaction of CH₄ + H₂O ⇌ CO + 3H₂ it's an endothermic reaction because the forward direction is endothermic, we know this because our H₂O and CH₄ molecules are no where to be seen, so they must've been broken and bond breaking is endothermic so our reaction is endothermic. An endothermic reaction has a positive △H because reactants have less energy than products because reactants lose energy to the products meaning the △H is positive. If temperature is increased the position of equilibrium shifts to the right. This is because an increase in temperature means the surroundings get hotter, an endothermic reaction absorbs heat, this will counteract the warmth. balancing it out, restoring equilibrium. So we want to shift the position of equilibrium to the endothermic direction. This is the right, so position of equilibrium shifts to the right. So more product is made.
0%
state the △H, decreased temperature change, energy of products and reactants and the type of reaction of CO + 2H₂ ⇌ CH₃OH it's an exothermic reaction because the backwards direction is endothermic and we know this because if we go from 1 substance to 2 substances you must've broken bonds, like if we have a whole pizza, and we split it into 2, now we have 2 bits, so we have broken the pizza, just like we have broken the bonds. Breaking bonds is endothermic as it needs energy. An exothermic reaction has a negative △H because reactants have more energy than products, so the energy must've been lost meaning the change of energy is negative. If temperature is decreased, position of equilibrium shifts to the right. This is because a decrease in temperature means the surroundings get colder, an exothermic reaction releases heat, this will counteract the cold, balancing it out, restoring equilibrium. So we want to shift the position of equilibrium to the exothermic direction. This is the right, so position of equilibrium shifts to the right. So more product is made.
0%
what is a characteristic of hydrogen peroxide it slowly and naturally decomposes to produce water and oxygen
0%
what is specific heat capacity measured in J/g°C
0%
what is △H measured in usually kJ/mol
0%
what is the catalyst we use in the decomposition hydrogen peroxide manganese (IV) oxide (MnO₂)
0%
describe how to carry out the experiment between Hydrochloric acid and calcium carbonate marble chips react with hydrochloric acid to give calcium chloride solution, water and carbon dioxide gas.1: put a beaker onto a mass balance 2: place hydrochloric acid in the beaker 3: place marble chips in the beaker containing HCl 4: put cotton wool instead of a bung on top of the beaker to stop acid spraying out and escaping, ruining the results and to allow carbon dioxide to escape so we can measure how much was lost 5: The change in mass of beaker is measured and put on a graph 6: the change in mass is the carbon dioxide escaping 7: This is because as marble chips react with the acid, carbon dioxide is released 8: the mass of carbon dioxide lost is measured and recorded at regular intervals
0%
what is calorimetry measures amount of energy transferred in a chemical reaction
0%
9999999999999999999 state the chemical equation for the production of magnesium sulfate from magnesium Mg + CuSO₄ ̣̣─> MgSO₄ + Cu
0%
what is the activation energy minimum amount of energy a chemical reaction needs in order to take place
0%
what does △H mean (molar) enthalpy change
0%
what can concentration be measured in mol/dm³ g/dm³
0%
what happens when the position of equilibrium shifts to the left moves away from productsmoves away from right moves towards left moves towards reactants produces less product produces more reactant balances everything out restores equilibrium happens when product is added or reactant is removed
0%
what happens when the position of equilibrium shifts to the right moves away from reactantsmoves away from left moves towards right moves towards products produces less reactant produces more product balances everything out restores equilibrium happens when reactant is added or product is removed
0%
does forming bonds need energy no
0%
what type of calcium carbonate should you use to get the slowest rate of reaction one big chunk of calcium carbonate
0%
what can't a catalyst affect in a reversible reaction position of equilibrium
0%
what happens when the conditions of an equilibrium reaction change position of equilibrium changes to counteract the change in conditions in order to restore eqauilibrium
0%
what does the position of equilibrium depend on pressure and temperature of reactants
0%
what happens when hydrogen chloride and nitrogen are cooled produces ammonium chloride
0%
what happens when ammonium chloride is thermally decomposed produces hydrogen chloride gas and nitrogen
0%
how does a catalyst work provides an alternative pathway for the reaction to take place with a lower activation energy so the reaction can happen
0%
state the formula for energy transferred Q= mc△T
0%
state the equations for the rate of reaction rate of reaction = mass of product formed / time rate of reaction = mass of reactant used / time
0%
why do reactants have less energy than products sometimes reactants absorb heat energy from surroundings which warms the products
0%
why do reactants have more energy than products sometimes reactants give heat energy to surroundings which warms the surroundings
0%
9999999999999999999 what is an endothermic reaction reaction that absorbs heat energy
0%
9999999999999999999 what is an exothermic reaction reaction that releases heat energy
0%
999999999999999999 what is a reversible reaction reaction where the forward and backward reactions happen at the same time
0%
what is the position of equilibrium relative concentrations of reactants and products
0%
what does an increase temperature do to position of equilibrium shifts to endothermic direction
0%
what does an decrease temperature do to position of equilibrium shifts to exothermic reaction
0%
what does an increase pressure do to position of equilibrium shifts to side that produces fewer gas molecules
0%
what does an decrease pressure do to position of equilibrium shifts to side that produces more gas molecules
0%
describe the combustion reaction of ethanol So, it combusts meaning it reacts with oxygen. This experiment measures how much energy is produced when a fuel is burnt. Our fuel is an alcohol and it is placed in a spirit burner. Use a thermometer to measure the temperature. The experiment goes as follows: First, the spirit burner containing the alcohol is measured both together as one mass and recorded. Then 100cm³ of water is transferred into a copper container and it's initial temperature is measured and recorded. The spirit burner is lit and placed under the copper container. The water heats up. Water is stirred constantly with the thermometer until the temperature rises by what you wanted, let's say it was 30°C. After this value is reached, extinguish the flame and measure and record the maximum temperature. Finally, the spirit burner containing the remaining alcohol is re weighed again collectively, then subtract the final mass from the initial mass to get the amount of alcohol burnt. Let's say our water was at room temperature, so if the change in temperature is 30°C then our final temperature is 50°C. Let's say the mass of the spirit burner and alcohol was 34.46g and after it was 32.57g then we do 34.46 - 32.57 to get 1.89. So 1.89g of alcohol was burnt. As we know the specific heat capacity of water is 4.2J/g °C we can work out the energy transferred. So Q = mc△T substitute the values in to get 100 x 4.2 x 30 = 12,600. This means 1.89g of alcohol burns to produce 12,600J of energy. We can work out how much energy is released when we burn 1g of our alcohol by doing 12,600 ÷ 1.89 = 6666.67. So about 6700J is released when we burn 1g of our alcohol. The word equation is: alcohol + oxygen ─> carbon dioxide + water
0%
what is c specific heat capacity
0%
what does a catalyst do in a reversible reaction speeds up the forward and backward direction
0%
what's a bond energy strength of a chemical bond
0%
what poisonous gas is produced during the reaction between sodium thiosulfate and hydrochloric acid and how do we prevent getting harmed sulfur dioxide is produced which dissolves in water to give an acidic solutionof sulfurous acid. The reaction is carried out in a well ventilated room so we don't get harmed.
0%
what is specific heat capacity the amount of energy needed to heat 1g of a substance by 1°C
0%
9999999999999999999 describe the table and graph of the reaction between sodium thiosulfate and hydrochloric acid when we vary the concentration of sodium thiosulfate the graph and table show that rate of reaction is directly proportional to concentration of sodium thiosulfate. This experiment can be repeated to show how temperature affects the rate of reaction, where we keep everything the same but just increase temperature.
0%
what will happen if you carry out the calcium carbonate and hydrochloric acid experiment but with bigger marble chips with a total mass of the same before, like you have joined the smaller marble chips together these bigger marble chips have a smaller surface area, so reaction will be slower. The same carbon dioxide is produced as it has the same mass, but it takes longer for it to reach the maximum carbon dioxide produced. So it takes longer for the line to plateau or become flat. It is less steep to begin, showing it's slower than before.
0%
what will happen if you carry out the calcium carbonate and hydrochloric acid experiment but with half the concentration of acid the volume and mass of acid stays the same it's just more diluted, otherwise the experiment would measure how much volume affects the rate of reaction. the marble chips need to be in excess, this reaction happens slower as they are less acid particles per unit of volume so the marble chip particles have to travel further to react so it takes longer. It produces exactly half the carbon dioxide as before and takes longer to reach the horizontal line which indicates the termination of the reaction.
0%
999999999999999999 how do we vary the concentration of sodium thiosulfate in the reaction between sodium thiosulfate and hydrochloric acid the volumes of water and sodium thiosulfate are varied. but the total volume of the 2 need to be kept the same otherwise we are looking at the effect of volume on the rate of reaction, but we want to look at the effect of concentration. The results are recorded and placed on a table and graph.
0%
9999999999999999999 how do we find the rate of reaction time ⁻¹ 1/time
0%
why do the reactants bonds need to be broken in a chemical reaction to make new bonds which forms the products
0%
99999999999999999 how can a reaction be endothermic if the total energy released equals the total absorbed total energy needed to break all bonds is different for every compound
0%
when is the reaction endothermic when the total energy needed to break bonds is higher than the total energy released by forming new bonds
0%
when is the reaction exothermic when the total energy released by making new bonds is higher than the total energy needed to break bonds
0%
what precipitate forms when sodium thiosulfate and hydrochloric acid react yellow sulfur precipitate
0%
can reactions have more gas molecules on one side yes
0%
does breaking bonds need energy yes
0%
do all bonds have a bond energy yes
0%
does the bond energy ever change yes, it changes slightly when it's bond is in a different compound
0%
No matching quizzes found
Score Distribution
Percent of People with Each Score
Percentile by Number Answered
Your Score History
You have not taken this quiz since the last reset
Copyright H Brothers Inc, 2008–2026
Contact Us | Go To Top | View Desktop Site | Site Map