A sample of hydrogen at 50◦C exerts a pressure of 0.377 atm. The gas is heated to 61◦C at constant volume. What will its new pressure be?

how do i find the pressure? i don't understand!!!!!!!!!!!

To find the new pressure of the hydrogen gas after it is heated, you can use the ideal gas law equation:

PV = nRT

Where:
P is the pressure of the gas
V is the volume of the gas
n is the number of moles of the gas
R is the ideal gas constant
T is the temperature of the gas (in Kelvin)

In order to use this equation, you need to convert the temperatures from Celsius to Kelvin.

To convert from Celsius to Kelvin, you use the formula:
T(K) = T(°C) + 273.15

First, let's convert the initial temperature from Celsius to Kelvin:

Initial temperature (T1) = 50°C
T1 (K) = 50 + 273.15 = 323.15 K

Next, convert the final temperature from Celsius to Kelvin:

Final temperature (T2) = 61°C
T2 (K) = 61 + 273.15 = 334.15 K

Since the volume remains constant, you can cancel it out from the equation:

P1/T1 = P2/T2

Now, plug in the values:

0.377 atm / 323.15 K = P2 / 334.15 K

Now, cross-multiply and solve for P2:

P2 = (0.377 atm × 334.15 K) / 323.15 K

P2 ≈ 0.390 atm

Therefore, the new pressure of the hydrogen gas will be approximately 0.390 atm when heated to 61°C at constant volume.