General Chemistry Answers

The combustion of toluene has a ΔErxn of −3.91 × 103kJ/mol. When 1.35 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 23.48 ∘C to 36.19 ∘C. Find the heat capacity of the bomb calorimeter. Express your answer using three significant figures.

How much heat is required to warm 1.60 L of water from 22.0 ∘C to 100.0? (Assume a density of 1.0g/mL for the water.)    

Express your answer in joules to two significant figures.

combustion of butane balanced equation how many moles of o2 are required to react completely with .35 mole of butane

The reaction 2 NO(g) ↔N2(g) + O2(g) has a Kc value of 2400 at 2000 K. If 0.850 M each of N2 and O2 are initially present in a 3.00-L vessel, calculate the equilibrium concentrations of NO, N2, and O2.

When 1.50 mol of CO2 and 1.50 mol H2 are placed in a 3.00-L container at 395ºC, the following reaction occurs: CO2(g) + H2(g) ↔ CO(g) + H2O(g).

If Kc = 0.802, what are the concentrations of each substance in the equilibrium mixture?

2 Al + 3 FeSO₃ -> Al₂(SO₃)₃ + 3 Fe

if 136 grams of aluminum are consumed, how many grams of iron are produced?

What mass of AlF₃ is produced when 168 grams of Al is consumed?

If 6.30 moles of AlF₃ are produced, what mass of F₂ is consumed?

Four moles of water molecules contains:

A) 

36 g of water

B) 

4.816 x 10²⁴ oxygen atoms

C) 

2.408 x 10²⁴ hydrogen atoms

D) 

2.408 x 10²⁴ molecules of water

Consider the unbalanced chemical reaction:  KO2 (s) + H2O(ℓ) →  KOH (s) + O2 (g) . 

If 10.70 g of KO2 and 1.80 g of H2O are reacted together:

a) What is the limiting reagent?

b) What mass of O2 can be produced?

c) Assuming the reaction takes place in a 1L vessel and the temperature is controlled at 25℃, what will the pressure of the vessel be?

d) If 2.22g of O2 is produced, what is the percent yield of the reaction?