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kvv77 [185]
3 years ago
6

WILL MARK BRANLIEST FOR CORRECT ANSWER! Given the following equation, write the expression for its relative rate.

Chemistry
1 answer:
USPshnik [31]3 years ago
7 0

\tt -\dfrac{1}{2}\dfrac{d[N_2O]}{dt}=\dfrac{1}{2}\dfrac{d[N_2]}{dt}=\dfrac{1}{1}\dfrac{d[O_2]}{dt}

<h3>Further explanation</h3>

Reaction

2N2O(g) — 2N2(g) + O2(g)

Required

relative rate

Solution

The reaction rate (v) shows the change in the concentration of the substance (changes in addition to concentrations for reaction products or changes in concentration reduction for reactants) per unit time.

so the relative rates for the reaction above are :

\tt -\dfrac{1}{2}\dfrac{d[N_2O]}{dt}=\dfrac{1}{2}\dfrac{d[N_2]}{dt}=\dfrac{1}{1}\dfrac{d[O_2]}{dt}

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Hope this helps! Tbh am not good at explaining. If u have any doubts, ask me!
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3 years ago
Colder air tends to have _____.
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Answer:

I believe the answer is D

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The table describes how some substances were formed.
Tanzania [10]

R is the mixture formed by adding 5 g of sugar to 1 L of water.

<h3>Which is a mixture?</h3>

A mixture is an impure substance made up of two or more substances which are miscible or immiscible in each other.

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Hence, R is the mixture formed by adding 5 g of sugar to 1 L of water.

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2 years ago
Calculate the mass of magnesium needed to make 25g of magnesium oxide​
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3 years ago
When 27.50 liters of oxygen gas reacts with excess hydrogen gas at STP how many grams of water is produced?
telo118 [61]

<u>Answer: </u>The mass of water produced is 44.28 g

<u>Explanation:</u>

We are given:

Volume of oxygen gas = 27.50 L

At STP conditions:

22.4 L of volume is occupied by 1 mole of a substance

27.50 L of oxygen gas will be occupied by = \frac{1mol}{22.4L}\times 27.50L=1.23mol

The chemical equation for the formation of water follows:

2H_2+O_2\rightarrow 2H_2O

By the stoichiometry of the reaction:

If 1 mole of oxygen gas produces 2 moles of water

So, 1.23 moles of oxygen gas will produce = \frac{2}{1}\times 1.23=2.46mol of water

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}} ......(1)

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Plugging values in equation 1:

\text{Mass of water}=(2.46mol\times 18g/mol)=44.28g

Hence, the mass of water produced is 44.28 g

5 0
3 years ago
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