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3 years ago

How do balanced chemical equations show the conservation of mass

Chemistry

2 answers:

antiseptic1488 [7]3 years ago

4 0

Answer: Matter cannot be created or destroyed

Explanation: Balanced equations are set equations we cannot change one element or compound in the equation without changing the entire equation. So balanced equation show the conservation of mass because while other substances may be formed from the synthesis or decomposition of compounds new elements are never introduced and are not created out of thin air :)

Rudiy273 years ago

3 0

Answer:

Matter cannot be created or destroyed in chemical reactions. This is the law of conservation of mass. In every chemical reaction, the same mass of matter must end up in the products as started in the reactants. Balanced chemical equations show that mass is conserved in chemical reactions.

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Predict whether the following reactions will be exothermic or endothermic.

Solnce55 [7]

Answer:

A. N₂(g) + 3H₂(g) -----> 2NH₃ exothermic

B. S(g) + O₂(g) --------> SO₂(g) exothermic

C. 2H₂O(g) --------> 2H₂(g) + O₂(g) endothermic

D. 2F(g) ---------> F₂(g) exothermic

Explanation:

The question says predict not calculate. So you have to use your chemistry knowledge, experience and intuition.

A. N₂(g) + 3H₂(g) -----> 2NH₃ is exothermic because the Haber process gives out energy

B. S(g) + O₂(g) --------> SO₂(g) is exothermic because it is a combustion. The majority, if not all, combustion give out energy.

C. 2H₂O(g) --------> 2H₂(g) + O₂(g) is endothermic because it is the reverse reaction of the combustion of hydrogen. If the reverse reaction is exothermic then the forward reaction is endothermic

D. 2F(g) ---------> F₂(g) is exothermic because the backward reaction is endothermic. Atomisation is always an endothermic reaction so the forward reaction is exothermic

5 0

3 years ago

1. Interpret the following equation using moles, molecules, and volumes (assume STP). Compare the mass of the reactants to the m

blsea [12.9K]

1. In this reaction, 2 moles of nitrogen gas reacts with 3 moles of oxygen gas to give 2 moles of N2O3 gas. 2 nitrogen molecules react with 3 oxygen molecules to give 2 N2O3 molecules. Under STP, one mole of an ideal gas occupies a volume of 22.4 liters. So in this reaction, 44.8 liters of nitrogen gas reacts with 67.2 liters of oxygen gas to give 44.8 liters of N2O3 gas. The total mass of the reactants (N2 and O2) is the same as the total mass of the product (N2O3). This is called mass balance of a chemical reaction.

2. According to the chemical reaction, 3 moles of chlorine gas produces 2 moles of iron(III) chloride. So, to produce 1 moles of iron(III) chloride, 3/2 (1.5) moles of chlorine gas is required. Therefore, to produce 14 moles of iron(III) chloride, 14 x 1.5 = 21 moles of chlorine is needed.

3 0

3 years ago

Read 2 more answers

What type of compound is fe3n2

Shkiper50 [21]

Fe3N2, also known as Iron (II) nitride, is an ionic compound.

Ionic compounds are compounds that consists of metals and non-metals bonded with ionic bonds. The metal ion gives up electron(s) to the non-metals.

Since iron is a metal and nitrogen is an non-metal, the bond they would form would be an ionic bond. Iron gives up 2 electrons to form iron(II) ion, while nitrogen gains 3 electrons to form nitride ion. Since one iron cannot let a nitrogen gain 3 electrons, so in the compound, there would be 3 iron (ii) ions that has given up 6 electrons in total while 2 nitride ions have gained 6 electrons in total.

8 0

3 years ago

How is the AHfusion used to calculate volume of liquid frozen that produces 1

yulyashka [42]

Answer:

option B

Explanation:

3 0

3 years ago

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A cylinder was charged with 1.25 atm of oxygen gas, 6.73 atm of argon, and 0.895 atm of xenon. What is the mole fraction of each

katrin2010 [14]

Considering the Dalton's partial pressure, the mole fraction of each gas is:

$x_{oxygen}$ = 0.14
$x_{argon}$ = 0.76
$x_{xenon}$ = 0.10

<h3>Dalton's partial pressure</h3>

The pressure exerted by a particular gas in a mixture is known as its partial pressure.

So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:

$P_{T} =P_{1} +P_{2} +...+P_{n}$

where n is the amount of gases in the gas mixture.

This relationship is due to the assumption that there are no attractive forces between the gases.

Dalton's partial pressure law can also be expressed in terms of the mole fraction of the gas in the mixture. The mole fraction is a dimensionless quantity that expresses the ratio of the number of moles of a component to the number of moles of all the components present.

So in a mixture of two or more gases, the partial pressure of gas A can be expressed as:

$P_{A} =x_{A} P_{T}$

In summary, the total pressure in a mixture of gases is equal to the sum of partial pressures of each gas.

Mole fraction of each gas

In this case, you know that:

$P_{oxygen }$ = 1.25 atm
$P_{argon}$ = 6.73 atm
$P_{xenon}$ = 0.895 atm
$P_{T} =P_{oxygen} +P_{argon}+P_{xenon}$ = 1.25 atm + 6.73 atm + 0.895 atm= 8.875 atm