Answer:
Explanation:
Hello!
In this case, since the undergoing chemical reaction is:

The equilibrium expression in terms of pressures is:

Thus, for the initial conditions, we compute the initial pressures of both nitric oxide and oxygen:

Next, since the equilibrium pressure is 1148 mmHg or 1.51 atm, we can write:

Thus, the Kp turns out:

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The malleable metal on the periodic table with the atomic number of 79 is gold
<h3>
Answer:</h3>
The pressure increases by 10% of the original pressure
Thus the new pressure is 1.1 times the original pressure.
<h3>
Explanation:</h3>
We are given;
- Initial temperature as 30°C, but K = °C + 273.15
- Thus, Initial temperature, T1 =303.15 K
- Final temperature, T2 is 333.15 K
We are required to state what happens to the pressure;
- We are going to base our arguments to Pressure law;
- According to pressure law, the pressure of a gas and its temperature are directly proportional at a constant volume
- That is; P α T
- Therefore, at varying pressure and temperature

Assuming the initial pressure, P1 is P
Rearranging the formula;
[tex]P2=\frac{P1T2}{T1}[/tex]


= 1.10 P
The new pressure becomes 1.10P
This means the pressure has increased by 10%
We can conclude that, the new pressure will be 1.1 times the original pressure.
B. We are in the cenzoic era so what previously had happen to cause the life we live today was a huge mass extinction.... hope this helps!!