A cylinder contains a moles of hydrogen at 0 degree celsius and 76cmHg.calculate the amount of heat require to raise the temperature of hudrogen to 50 degree celcius.keeping the pressure constant and what is the volume of hydrogen when at 0 degree celsius.
Q = nc change T
You'll need to look up the specific heat of H2 and use a number instead of "a" for the moles.
V = nRT/P Be sure to convert to Kelvins and find a unit suitable R.
To calculate the amount of heat required to raise the temperature of hydrogen at constant pressure, we can use the equation:
Q = n * Cp * ΔT
where:
Q = amount of heat (in Joules)
n = number of moles of hydrogen
Cp = molar heat capacity of hydrogen at constant pressure (approximately 28.8 J/mol°C)
ΔT = change in temperature (in °C)
First, let's calculate the initial volume of hydrogen at 0°C. From the ideal gas law, we know that:
PV = nRT
where:
P = pressure (in cmHg) = 76 cmHg
V = volume (in liters)
n = number of moles of hydrogen
R = ideal gas constant = 0.0821 L.atm/mol.K
T = temperature (in Kelvin)
To convert 0°C to Kelvin, we add 273.15:
T(initial) = 0°C + 273.15 = 273.15 K
Now, let's calculate the volume of hydrogen:
PV = nRT
76 cmHg * V = n * 0.0821 L.atm/mol.K * 273.15 K
V = n * 0.0821 * 273.15 / 76
V = n * 0.2954
Therefore, the volume of hydrogen at 0°C is V = n * 0.2954 liters.
Next, to calculate the amount of heat required to raise the temperature to 50°C, we substitute the values into the equation:
Q = n * Cp * ΔT
Q = n * 28.8 J/mol°C * (50°C - 0°C)
Q = n * 28.8 J/mol°C * 50°C
Now, to calculate the amount of heat required, we need to know the value of n (number of moles of hydrogen). If you provide the number of moles, we can continue with the calculation.