Show all your work

Write the reaction between solid zinc (II) bisulfite and aqueous hydroiodic acid.

Assume ∆H = -500.0 KJ/mol zn (II) bisulfite, and the reaction occurs under constant pressure.

During this reaction a gas was produced. If 200. m3 of gas was produced at a temperature of 98.0⁰F and 1.07 atm, calculate the amount of heat (KJ) produced.

answer

watching

573

views

For unlimited access to Homework Help, a Homework+ subscription is required.

Liked by manya12 and 6 others

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

fuchsiawallaby436Lv1

11 Jun 2021

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

When 1 mol of iron metal reacts with hydrochloric acid at constant temperature and pressure to produce hydrogen gas aqueous iron (II) chloride, 89.1 kJ of heat evolves. Write a thermochemical equation for this reaction.

ivoryminnow72

Consider the following reaction.CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ(a) the reaction is endothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.answer isH = 113.23 kJ (c) If the enthalpy change is 17.0 kJ, how many grams of hydrogen gas are produced? answer is .757 g (d) How many kilojoules of heat are released when 14.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure? answer isH = -45.3 kJ (e) Calculate delta E when 500.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K ???? I've already tried 85.7, 1624, and 1614. I am so lost