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5 mole of hydrogen gas is heated from 30ºC to 60ºC at constant pressure. Heat given to the gas is in calories (given R = 2cal/mole-ºC)
    Correct answer is '1050'. Can you explain this answer?
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    5 mole of hydrogen gas is heated from 30ºC to 60ºC at consta...




    = 1050 calories
    The correct answer is: 1050
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    5 mole of hydrogen gas is heated from 30ºC to 60ºC at consta...
    To solve this problem, we can use the ideal gas law equation:

    PV = nRT

    Where:
    P = pressure (in atm)
    V = volume (in liters)
    n = number of moles
    R = ideal gas constant (0.0821 L·atm/(mol·K))
    T = temperature (in Kelvin)

    First, let's convert the given temperature from Celsius to Kelvin:
    30°C + 273.15 = 303.15 K

    Now, we can rearrange the ideal gas law equation to solve for volume:
    V = (nRT)/P

    Given:
    n = 5 moles
    T = 303.15 K
    P = unknown

    We need to find the pressure (P), so we rearrange the equation further:
    P = (nRT)/V

    Now, substitute the given values into the equation:
    P = (5 moles * 0.0821 L·atm/(mol·K) * 303.15 K) / V

    Since we don't have the volume (V) given in the question, we can't calculate the pressure accurately. The volume is necessary to solve the problem.
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    5 mole of hydrogen gas is heated from 30ºC to 60ºC at constant pressure. Heat given to the gas is in calories (given R = 2cal/mole-ºC)Correct answer is '1050'. Can you explain this answer?
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