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3 years ago

How do you calculate the mass of a product when the amounts of more than one reactant are given?

1 answer:

3 0

you add the masses of the reactants, because of conservation of mass. if there are two or more products they will ask you to find the mass of only one product or the sum of the mass of all products

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The activation energy for a given reaction is 56 kj/mol. at what temperature would the rate constant be quadruple what is was at

Alex787 [66]

The rate equation is given as:

k = A e^(- Ea / RT)

Dividing state 1 and state 2:

k1/k2 = e^(- Ea / RT1) / e^(- Ea / RT2)

k1/k2 = e^[- Ea / RT1 - (- Ea / RT2)]

k1/k2 = e^[- Ea / RT1 + Ea / RT2)]

Taking the ln of both sides:

ln (k1/k2) = - Ea / RT1 + Ea / RT2

ln (k1/k2) = - Ea / R (1/T1 - 1/T2)

Since k2 = 4k1, therefore k1/k2 = ¼

ln (1/4) = [- (56,000 J/mol) / (8.314 J / mol K)] (1/273 K – 1/ T2)

2.058 x 10^-4 = 1/273 – 1/T2

T2 = 289.25 K

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3 years ago

Once the sun's energy reaches the earth's atmosphere through radiation, it is circulated within the atmosphere and oceans throug

maw [93]

The sun's energy would be circulated through convection. This is because whenever you see the word "circulate", there is a pretty good chance it has something to do with convection.

5 0

4 years ago

Read 2 more answers

In 1909 Fritz Haber discovered the workable conditions under which nitrogen, N2(g), and hydrogen, H2(g), would combine using to

labwork [276]

Answer : 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

Solution : Given,

Mass of $NH_3$ = 100 g

Molar mass of $NH_3$ = 27 g/mole

Molar mass of $N_2$ = 28 g/mole

First we have to calculate moles of $NH_3$ .

$\text{ Moles of }NH_3=\frac{\text{ Mass of }NH_3}{\text{ Molar mass of }NH_3}= \frac{100g}{27g/mole}=3.7moles$

The given balanced chemical reaction is,

$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$

From the given reaction, we conclude that

2 moles of $NH_3$ produced from 1 mole of $N_2$

3.7 moles of $NH_3$ produced from $\frac{1mole}{2mole}\times 3.7mole=1.85moles$ of $N_2$

Now we have to calculate the mass of $N_2$ .

Mass of $N_2$ = Moles of $N_2$ × Molar mass of $N_2$

Mass of $N_2$ = 1.85 mole × 28 g/mole = 51.8 g

Therefore, 51.8 g of nitrogen are needed to produce 100 grams of ammonia gas.

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3 years ago

What is meant by “normal” when you are asked for normal boiling and melting points?

RideAnS [48]

Answer:

Normal boiling point is the temperature at which a liquid boils at 1 atmosphere of pressure.

Explanation:

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3 years ago

Elements that have five electrons in the highest-energy p sublevel in their ground state are called what?

wolverine [178]

Elements that have six electrons in the highest-energy p sublevel in their ground state are called the noble gases or inert gases. The six noble gases that occur naturally are helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and the radioactive radon (Rn).

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3 years ago