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riadik2000 [5.3K]
2 years ago
15

What is the relationship between a chemical equation and a chemical reaction? What are reactants and products in a chemical equa

tion?​
Chemistry
1 answer:
Sergio039 [100]2 years ago
5 0

Answer:

A chemical reaction occurs when reactants are converted into products. A chemical equation is a representation of a chemical reaction using chemical symbols. The chemical equation also indicates the physical state of the reactants and products. The substances that go into a chemical reaction are called the reactants, and the substances produced at the end of the reaction are known as the products.

Explanation: because UwU

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8 0
3 years ago
What mass of chromium would be produced from the reaction of 57.0 g of potassium with 199 g of chromium(II) bromide according to
fredd [130]

Answer:

Mass of Chromium produced = 37.91 grams

Explanation:

2K + CrBr₂  →  2KBr + Cr

2mole     1 mole                1 mole

mass of Potassium = 57.0 grams

molar mass of Potassium = 39.1 g/mol

no of moles of Potassium = 57.0 / 39.1 = 1.458 moles

mass of CrBr₂= 199 grams

molar mass of CrBr₂ = 211.8 gram/mole

no of moles of CrBr₂ = 199 / 211.8 = 0.939 mole

From chemical equation

1 mole of CrBr₂ = 2 moles of K

∴ 0.939 moles of CrBr₂ = ?

   ⇒ 0.939 x 2/1 = 1.878 moles of K

1.878 moles of K is needed, but there is 1.458 moles of K. So, Potassium is completed first during the reaction . Hence, Potassium is limiting reagent. and CrBr₂ is excess reagent .

From chemical equation

2 moles of K = 1 mole of Cr

∴ 1.458 moles of K = ?

   ⇒ 1.458 x 1/ 2 = 0.729 moles of Cr

no of moles of Cr formed = 0.729 moles

molar mass of Cr = 52.0 g/mol

mass of one mole of Cr = 52.0 grams

mass of 0.729 moles of Cr = 52.0 x 0.729 = 37.908 grams

mass of Chromium produced = 37.91 grams

6 0
3 years ago
A sample of ethanol (C2H5OH), weighing 6.83 g underwent combustion in a bomb calorimeter by the following reaction: C2H5OH (l) +
iren [92.7K]

The question is incomplete, here is the complete question.

A sample of ethanol (C_2H_5OH), weighing 6.83 g underwent combustion in a bomb calorimeter by the following reaction:

C_2H_5OH(l)+3O_2(g)\rightarrow 2CO_2(g)+3H_2O(l)

If the heat capacity of the calorimeter and contents was 18.1 kJ/°C and the temperature of the calorimeter rose from 25.50°C to 36.73°C. What is the \Delta H of the reaction?

<u>Answer:</u> The enthalpy of the reaction is -1355.1 kJ

<u>Explanation:</u>

To calculate the heat absorbed by the calorimeter, we use the equation:

q=c\Delta T

where,

q = heat absorbed

c = heat capacity of calorimeter = 18.1 kJ/°C

\Delta T = change in temperature = T_2-T_1=(36.73-25.50)^oC=11.23^oC

Putting values in above equation, we get:

q=18.1kJ/^oC\times 11.23^oC=203.26kJ

Heat absorbed by the calorimeter will be equal to the heat released by the reaction.

<u>Sign convention of heat:</u>

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Given mass of ethanol = 6.83 g

Molar mass of ethanol = 46 g/mol

Putting values in above equation, we get:

\text{Moles of ethanol}=\frac{6.83g}{46g/mol}=0.15mol

To calculate the enthalpy change of the reaction, we use the equation:

\Delta H_{rxn}=\frac{q}{n}

where,

q = amount of heat released = -203.26 kJ

n = number of moles = 0.15 moles

\Delta H_{rxn} = enthalpy change of the reaction

Putting values in above equation, we get:

\Delta H_{rxn}=\frac{-203.26kJ}{0.15mol}=-1355.1kJ/mol

Hence, the enthalpy of the reaction is -1355.1 kJ

7 0
3 years ago
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