A reaction at 34.0 °C evolves 436. mmol of boron trifluoride gas. Calculate the volume of boron trifluoride gas that is collected. You can assume the pressure in the room is exactly 1 atm. Round your answer to 3 significant digits.

Given:  Temperature of H2O = 200C Pressure = 0.95 atm Initial Air Volume = 50mL Final Air Volume = 95mL Volume of O2 collected = 95mL - 50mL = 45mL Total Reaction time = 17mins Balanced equation for hydrogen peroxide decomposition: 2H2O2  ------ 2H2  +   O2 Using the Ideal Gas Law (PV = nRT), calculate the grams of O2 produced in the reaction above(decomposition of hydrogen peroxide). (Hint: solve for n, and then convert moles of O2 to grams. Watch your units; you may need to convert some of your data into different units.)

explain the parr adiabatic bomb calorimete

Acetic acid and ethanol react to form ethyl acetate and water, like this: HCH,CO,(aq)+C2H;OH(aq) →C,H;CO,CH3(aq)+H,O() Imagine 217. mmol of C,H,CO,CH, are removed from a flask containing a mixture of HCH,CO,, C,H,OH, C,H,CO,CH, and H,O at equilibrium, and then answer the following questions. O Zero. What is the rate of the reverse reaction before any C2H5CO,CH3 O Greater than zero, but less than the rate of the forward reaction. has been removed from the flask? O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse reaction just after the C,H5CO,CH3 has been removed from the flask? O Greater than zero, but less than the rate of the forward reaction. O Greater than zero, and equal to the rate of the forward reaction. O Greater than zero, and greater than the rate of the forward reaction. O Zero. What is the rate of the reverse reaction when the system has again…

The total pressure for this reaction is 1.4 torr: CH4(g) reacts with O2(g) to make CO2(g) and H2O(g) Calculate the partial pressure of H2O(g)

Sample Experimental Values: Reaction 1: Both reactants are 2M Reaction 2: Both Reactants are 2M NaOH (aq) + HCl (aq) → H₂O (1) + NaCl (aq) 1 Reaction 2 NaOH (aq) + CH3COOH (aq) → H₂O (1) + NaCH3COO (aq) Temperature Change 20 C 8 C Volume of Reactants 25.0 mL NaOH 25.0 mL HCI 10.0 mL NaOH 10.0 mL CH3COOH Final Mass of Solution 50.0 g 20.0 g 2. Using the sample experimental values, answer the questions below. a. Show the calculation used to determine how much heat was produced for both reactions. Report your answer in Joules. b. How much heat was released per mole of acid? (Hint: think about the concentration of the reactants and their respective volumes used. Report answer for both reactions in kJ/mol) What is the vocabulary chemists use to describe this experimental value? 3. Based on the experimental evidence, how is the heat of neutralization related to the strength of the acid?

Temperature of a sample containing 1 mole of neon is increased at constant pressure from 20 oC to 30 oC . Determine H for the sample during this process (treat argon as a perfect gas).

The reaction below generate 0.025moles of H2. If the gas is collected by displacing water in a large beaker, what is the total volume of gas in the breaker if the atmosphere pressure is 0.899atm and the temperature of the water and beaker is 35 Celsius? 2Al+2NaOH+2H2O=2NaAlO2+3H2

Chemistry 6CO2 + 6H₂O → C6H12O6 +602 Calculate ASrxn ASrxno for this reaction. Express your answer in joules per kelvin. O Calculate AG rxn AGrxn for this reaction at 35 C. C. Assume that AH rxn AHrxnᵒ and ASixn ASrxn° do not depend on temperature. Express your answer in kilojoules.

CaCO3(s)⇄CaO(s)+CO2(g) When heated strongly, solid calcium carbonate decomposes to produce solid calcium oxide and carbon dioxide gas, as represented by the equation above. A 2.0mol sample of CaCO3(s)is placed in a rigid 100.L1 reaction vessel from which all the air has been evacuated. The vessel is heated to 898°C898°C at which time the pressure of CO2(g) in the vessel is constant at 1.00atm1.00atm, while some CaCO3(s)remains in the vessel. (a) Calculate the number of moles of CO2(g) present in the vessel at equilibrium. b) Write the expression for Kp, the equilibrium constant for the reaction, and determine its value at 898°C (c) The experiment was repeated, but this time starting with a 4.0mol sample of CaCO3(s) On the following graph, draw a curve showing how the pressure of CO2(g)would change over time as the vessel is heated to 898°C  and equilibrium is established.