Nitrogen gas is stored at 200 kPa and 100 K in a rigid tank with a volume of 0.5 m3. If the temperature of the gas is increased to 400 K, what is the final pressure in the tank (answer in kPa)?

The final temperature is 800KPa

Explanation:

The following were obtained from the question:

P1 = 200 kPa

T1 = 100 K

T2 = 400 K

P2 =?

Since the tank is rigid, the volume of the tank is constant.

Using P1/T1 = P2/T2, we can obtain the new pressure as illustrated below:

200/100 = P2 /400

Cross multiply to express in linear form:

100 x P2 = 200 x 400

Divide both side by 100

P2 = (200 x 400) /100

P2 = 800KPa

The final temperature is 800KPa

a. patterns can explain observations.

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol