# Chemistry

N2O5 is an unstable gas that decomposes according to the following reaction:
2N2O3(g) ---> 4NO2(g) + O2(g)
What would be the total pressure of gases present if a 10.0L container at 22.0 degree centigrade begins with 0.400 atm of N2O5 and the gas completely decomposes?

1. 👍
2. 👎
3. 👁
1. You made a typo on the equation.
2N2O5 ==> 4NO2 + O2
When using gases one may use the gas pressure as if it were mols.
Convert atm N2O5 to atm NO2. That's 0.4 atom x (4 mols NO2/2 mols N2O5) = ? atm for NO2.
0.4 atm x (1 mol O2/2 mols N2O5) - ? atm for O2.

1. 👍
2. 👎
2. 1 atm

1. 👍
2. 👎

## Similar Questions

1. ### chemistry

Calculate ∆H0 for the reaction 2 N2(g) + 5 O2(g) −→ 2 N2O5(g) given the data H2(g) + 1 2 O2(g) −→ H2O(ℓ) ∆H0 f = −290 kJ/mol N2O5(g) + H2O(ℓ) −→ 2 HNO3(ℓ) ∆H0 = −77.8 kJ/mol 1 2 N2(g) + 3 2 O2(g) + 1 2

2. ### ap chem

A student collected concentration data to determine the rate of the decomposition of N2O5 to NO2 and O2. The data were recorded in the table below. What is the rate law of this reaction? A. k[NO2] B. k[N2O5] C. k D. k[N2O5]2

3. ### Chemistry

The mechanism for the reaction described by 2N2O5(g) ---> 4NO2(g) + O2(g) is suggested to be (1) N2O5(g) (k1)--->(K-1) NO2(g) + NO3(g) (2) NO2(g) + NO3(g) --->(K2) NO2(g) + O2(g) + NO(g) (3) NO(g) + N2O5(g) --->(K3) 3NO2(g)

4. ### chemistry

A student performed two side-by-side reactions to test the decomposition of N2O5. The only difference between the two reactions was reactant concentration — reaction 1 started with 2 M N2O5 and reaction 2 started with 1.2 M.

1. ### chemistry

Copper(II) nitrate decomposes upon heating to form copper(II) oxide, nitrogen dioxide gas, and oxygen gas. If 1.0 mole of copper(II) nitrate decomposes, how many moles of nitrogen dioxide would be formed?

2. ### Chemistry

Dinitrogen pentoxide, N2O5, decomposes by first-order kinetics with a rate constant of 0.15 s-1 at 353 K. (a) What is the half-life (in seconds) for the decomposition of N2O5 at 353 K? (b) If [N2O5]0 = 0.0579 mol·L-1, what will

3. ### chemistry

Write word equations for the following chemical reactions. a. Pure copper can be produced by heating copper(II) sulfide in the presence of diatomic oxygen from the air. Sulfur dioxide gas is also produced in this reaction. b.

4. ### CHE1

Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.60 g of hydrogen peroxide

1. ### Chemistry

Consider the following two thermochemical equations N2+2.5O2-> N2O5(s) Delta H=xkJ N2+2.5O2-> N2O5(g) Delta H=ykJ The enthalpy change in kJ for the sublimation of one mole of N205 solid to gas would be represented by the quantity

2. ### Science

A sample of water decomposes to make 4g of hydrogen gas and 32g of oxygen gas. What mass of water decomposed? How do you know? Hint: The water decomposes into ONLY hydrogen and oxygen, and the total mass does not change in the

3. ### chemistry

Calculate ∆H0 for the reaction 2 N2(g) + 5 O2(g) −→ 2 N2O5(g) given the data H2(g) + 1 2 O2(g) −→ H2O(ℓ) ∆H0 f = −283 kJ/mol N2O5(g) + H2O(ℓ) −→ 2 HNO3(ℓ) ∆H0 = −78.7 kJ/mol 1 2 N2(g) + 3 2 O2(g) + 1 2

4. ### Chemistry

How much oxygen (in grams) will form from 44.2 mg of N2O5? 2N2O5(s) → 4NO2(g) + O2(g) ____× 10^-3(g) O2