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2 years ago

Pressure of an ideal gas ___________________, when number of particles ( moles ) of gas decreases.

Chemistry

1 answer:

atroni [7]2 years ago

3 0

The answer to your question is B.

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An acid

tekilochka [14]

The answer is A. Has a low pH in solution.

5 0

2 years ago

The second-order rate constants for the reaction of oxygen atoms witharomatic hydrocarbons have been measured (R. Atkinson and J

Pepsi [2]

Answer:

A = 1,13x10¹⁰

Ea = 16,7 kJ/mol

Explanation:

Using Arrhenius law:

ln k = -Ea/R × 1/T + ln(A)

You can graph ln rate constant in x vs 1/T in y to obtain slope: -Ea/R and intercept is ln(A).

Using the values you will obtain:

y = -2006,9 x +23,147

As R = 8,314472x10⁻³ kJ/molK:

-Ea/8,314472x10⁻³ kJ/molK = -2006,9 K⁻¹

<em>Ea = 16,7 kJ/mol</em>

Pre-exponential factor is:

ln A = 23,147

A = e^23,147

I hope it helps!

6 0

2 years ago

Paul determines that the hydrogen ion concentration of his unknown solution is 3.60×10^-5 M. what is the pH of this solution?

vivado [14]

Answer:

Explanation:

The pH of a substance can be found by using the formula

$p H = - log[ H^{ + } ]$

where [ H+ ] is the hydrogen ion concentration of the solution

From the question

[ H + ] = 3.60 × 10^-5 M

So the pH is

$pH = - log(3.60 \times {10}^{ - 5} ) \\ =4.44369749923$

We have the final answer as

Hope this helps you

4 0

2 years ago

Can you substitute evaporated milk for condensed milk

alex41 [277]

Yes because condensed milk and evaporated milk are similar to one another. However, there won’t be the same sweet flavor but the texture is the same.

3 0

2 years ago

Calculate the number of pounds of CO2 released into the atmosphere when a 22.0 gallon tank of gasoline is burned in an automobil

IrinaK [193]

Answer:

391.28771 pounds of carbon-dioxide released into the atmosphere.

Explanation:

Density of the gasoline ,d= 0.692 g/mL

Volume of gasoline in an tanks,V = 22.0 gallons = 83,279.02 mL

Let mass of the gasolin be M

$d=\frac{M}{V}$

M = V × d = 83,279.02 mL × 0.692 g/mL=57,629.081 g

Assume that gasoline is primarily octane (given)

$2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O$

Mass of octane burnt in the tank = M = 57,629.081 g

Moles of octane = $\frac{57,629.081 g}{114.08 g/mol}=505.1637 mol$

According to reaction, 2 moles of octane gives 16 moles of carbon-dioxide.

Then 505.1637 mol of octane will give:

$\frac{16}{2}\times 505.1637 mol=4,041.3100 mol$ of carbon-dioxide

Mass of 4,041.3100 mol of carbon-dioxide:

4,041.3100 mol × 44.01 g/mol = 177,858.05 g

Mass of carbon-dioxide produced in pounds = 391.28771 pounds

391.28771 pounds of carbon-dioxide released into the atmosphe

4 0

3 years ago