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3 years ago

Identify the type of reaction, write the products with phases, and balance. Show all work.

1 answer:

8 0

The correct classification of the reactions are as follows:

<span>1) 2Mg(s) + O2(g)----> 2MgO (s)
It is a synthesis reaction or a combination reaction. It involves the bonding of the reactant molecules forming one single molecule with new set of properties.

2) Na(s) + Cl2(g)------> NaCl(s)
It is a combination reaction as well, the same as the first reaction.

3). PbCO3(s)------> PbO(s)+Co2(g)
It is a decomposition reaction where a single molecule is breaks down into multiple molecules.

4). Ch4(g) + 2O2(g)----> CO2(g) + 2H2O(g)
It is a combustion reaction since it involves the reaction with oxygen and the production od carbon dioxide and water.</span>

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A sample of cacl2⋅2h2o/k2c2o4⋅h2o solid salt mixture is dissolved in ~150 ml de-ionized h2o. the oven dried precipitate has a ma

Paraphin [41]

We are given that the balanced chemical reaction is:

cacl2⋅2h2o(aq) + k2c2o4⋅h2o(aq) ---> cac2o4⋅h2o(s) + 2kcl(aq) + 2h2o(l)

We known that the product was oven dried, therefore the mass of 0.333 g pertains only to that of the substance cac2o4⋅h2o(s). So what we will do first is to convert this into moles by dividing the mass with the molar mass. The molar mass of cac2o4⋅h2o(s) is molar mass of cac2o4 plus the molar mass of h2o.

molar mass cac2o4⋅h2o(s) = 128.10 + 18 = 146.10 g /mole

moles cac2o4⋅h2o(s) = 0.333 / 146.10 = 2.28 x 10^-3 moles

Looking at the balanced chemical reaction, the ratio of cac2o4⋅h2o(s) and k2c2o4⋅h2o(aq) is 1:1, therefore:

moles k2c2o4⋅h2o(aq) = 2.28 x 10^-3 moles

Converting this to mass:

mass k2c2o4⋅h2o(aq) = 2.28 x 10^-3 moles (184.24 g /mol) = 0.419931006 g

Therefore:

The mass of k2c2o4⋅<span>h2o(aq) in the salt mixture is about 0.420 g</span>

3 0

3 years ago

Read 2 more answers

Consider the following system at equilibrium where \Delta H° = 18.8 kJ, and Kc = 9.52×10-2, at 350 K.

slega [8]

Answer:

1. C. remains the same. 2. C. is less than Kc. 3. B. run in the reverse direction to reestablish equilibrium. 4. A. increase.

Explanation:

At constant temperature, the equilibrium concentration has not effect on the equilibrium constant because the rate constants do not change with change in the concentrations or amounts of the reactants or products. Change in the concentration of one reactant or product causes the concentration of the others to change so as to maintain a constant value for the equilibrium constant. On the other hand, the reaction quotient is used to measure the relative amounts of reactants and products during a chemical reaction at any point in time. The value of the reaction quotient shows the direction of the chemical reaction.

Therefore, when 0.31 moles of CCl4(g) are removed from the equilibrium system at constant temperature:

1. the value of Kc remains the same

2. the value of Qc is less than Kc

3. the reaction must run in the reverse direction to reestablish equilibrium

4. the concentration of $CH_{4}$ will increase because product will be converted to reactants to reestablish equilibrium.

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Aliun [14]

Answer:

Chemical reaction, compound, molecule, covalent bonds, ionic bonds, ions. (first page)

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Explanation:

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lara31 [8.8K]

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4 years ago

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baherus [9]

Answer:

D. Carbon dioxide

Explanation:

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3 years ago

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