What is the pressure, in atmospheres, if the gas is warmed to a temperature of 34 deg C and if V and n do not change? Express your answer to two significant figures and include the appropriate units.
To determine the pressure, we can use the ideal gas law, which states:
PV = nRT
Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
To convert 34°C to Kelvin, we add 273.15.
T = 34°C + 273.15 = 307.15 K
Since V and n do not change, we can rewrite the equation as:
P1V1 = P2V2
Since V and n are constant, V1 = V2 and n1 = n2.
So, P1 = P2
Therefore, the pressure remains unchanged.
The pressure, in atmospheres, remains the same.
To answer this question, you can use the ideal gas law equation, which is expressed as:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
To find the pressure, we need to rearrange the equation to solve for P. The rearranged equation would be:
P = (nRT) / V
Since the question states that V and n do not change, we can ignore them and focus on the temperature:
P = (RT) / V
Now, we can plug in the values into the equation. The ideal gas constant, R, is given as 0.0821 L(atm)/(mol*K). The temperature, T, is given as 34 °C, which needs to be converted to Kelvin by adding 273.15 to the Celsius temperature:
T = 34 °C + 273.15 = 307.15 K
Using these values, we can calculate the pressure:
P = (0.0821 L(atm)/(mol*K)) * (307.15 K) / V
Since the question does not provide a specific value for V, we cannot calculate the specific pressure. However, you can substitute the given value of V into this equation to find the pressure in atmospheres.
To find the pressure, we can use the ideal gas law equation, which states that the product of pressure (P), volume (V), and the number of moles of gas (n) is proportional to the temperature (T) in Kelvin (K):
PV = nRT
where R is the ideal gas constant.
We can start by converting the given temperature of 34°C to Kelvin. To do that, we need to add 273.15 to 34°C:
T(K) = 34°C + 273.15 = 307.15 K
Since the volume (V) and the number of moles (n) do not change, we can keep them constant and rearrange the ideal gas law equation to solve for pressure:
P = nRT / V
Since V and n are constant, we can simplify the equation to:
P = (constant) * T
This means that pressure is directly proportional to temperature when volume and moles are constant. Therefore, if the temperature increases, the pressure will also increase.
Since we are not given any specific values for V, n, or the gas constant R, we can't determine the exact pressure. However, we can still provide a general explanation.
To find the pressure, you would need to know the specific values for V, n, and R. Given that these values are not provided in the question, it is not possible to calculate the exact pressure. Therefore, the best we can do is explain the relationship between pressure and temperature, keeping V and n constant.