Q must be supplied = 119523.3~J
<h3>Further explanation </h3>
The law of conservation of energy can be applied to heat changes, i.e. the heat received/absorbed is the same as the heat released
Q in = Q out
Heat can be calculated using the formula:
Q = mc∆T
Q = heat, J
m = mass, g
c = specific heat, joules / g ° C
∆T = temperature difference, ° C / K
So from the question :
Q to the system(Q supplied) = Q water + Q steel vessel(Q gained)
Answer:
Mass = 36.4 ×10⁻³ g
Explanation:
Given data:
Volume of container = 100 mL ( 100/1000 = 0.1 L)
Pressure = 688 mmHg (0.9 atm)
Temperature = 565°C ( 565 + 273 = 838 K)
Mass in grams of nitrogen = ?
Solution:
According to ideal gas equation,
PV = nRT
n = number of moles
P = pressure
R = general gas constant
T = temperature
From this equation we will determine the number of moles and then we we will calculate the mass.
n = PV/RT
n = 0.9 atm × 0.1 L / 0.0821 atm. L / mol.K × 838 K
n = 0.09 / 68.8
n = 0.0013 mol
or
n = 1.3×10⁻³ mol
Mass of nitrogen gas:
Mass = number of moles × molar mass
Mass = 1.3×10⁻³ mol × 28 g/mol
Mass = 36.4 ×10⁻³ g
Answer: 1.09 kPa
Explanation:
Given that,
Original volume V1 = 3.2 L
Original pressure P1 = 2.8 kPa
New pressure P2 = ?
New volume V2 = 8.1 L
Since pressure and volume are given While temperature is constant, apply Boyle's law
P1V1 = P2V2
2.8 kPa x 3.2L = P2 x 8.1L
8.96 kPa L = P2 x 8.2L
P2 = 8.96 kPa L / 8.2L
P2 = 1.09 kPa
Thus, the pressure of the gas would be 1.09 kPa
James D Watson and Francis Crick
The reaction is at the equilibrium where Q=Keq