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Afina-wow [57]
2 years ago
11

An 18-g sample of element A combines completely with a 4-g sample of element B to form the compound AB. What is the mass of the

compound formed?
Chemistry
1 answer:
DaniilM [7]2 years ago
6 0

Answer:

22g

Explanation:

Given parameters:

Mass of element A = 18g

Mass of element B  = 4g

Unknown:

Mass of compound formed = ?

Solution:

 The reaction equation is given as;

          A   +   B   →  AB

According to the law of conservation of mass "in a chemical reaction, matter is neither created nor destroyed but changed from one form to another".

Simply mas is conserved and the mass of the reactants is the same as the mass of the product that forms.

  Mass of reactants  = mass of A + mass of B = 18g + 4g  = 22g

 So;

  Mass of product AB = 22g

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Answer:

The answer to this would be communicating.

Explanation:

A scientist would be communicating to his or her fellow colleagues and sharing to them his or her idea.

Hope you find this answer helpful! :)

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Chemically combined substances, such as CO2, NH3, and H20 are called.....
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It is d. compounds because they have more than one element.
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If we know this is a second-order reaction, what is the rate law?
Pavel [41]

Answer:

The rate is a mathematical relationship obtained by comparing reaction rate with reactant concentrations.

6 0
3 years ago
How many molecules are in
diamong [38]

Answer:

3.6 × 10²⁴ molecules

Explanation:

Step 1: Given data

Moles of methane (n): 6.0 moles

Step 2: Calculate the number of molecules of methane in 6.0 moles of methane

In order to convert moles to molecules, we need a conversion factor. In this case, we will use Avogadro's number: there are 6.02 × 10²³ molecules of methane in 1 mole of molecules of methane.

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6 0
3 years ago
Given these reactions, X ( s ) + 1 2 O 2 ( g ) ⟶ XO ( s ) Δ H = − 668.5 k J / m o l XCO 3 ( s ) ⟶ XO ( s ) + CO 2 ( g ) Δ H = +
qwelly [4]

<u>Answer:</u> The \Delta H^o_{rxn} for the reaction is -1052.8 kJ.

<u>Explanation:</u>

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

X(s)+\frac{1}{2}O_2(g)+CO_2(g)\rightarrow XCO_3(s)      \Delta H^o_{rxn}=?

The intermediate balanced chemical reaction are:

(1) X(s)+\frac{1}{2}O_2(g)\rightarrow XO(s)    \Delta H_1=-668.5kJ

(2) XCO_3(s)\rightarrow XO(s)+CO_2     \Delta H_2=+384.3kJ

The expression for enthalpy of the reaction follows:

\Delta H^o_{rxn}=[1\times \Delta H_1]+[1\times (-\Delta H_2)]

Putting values in above equation, we get:

\Delta H^o_{rxn}=[(1\times (-668.5))+(1\times (-384.3))=-1052.8kJ

Hence, the \Delta H^o_{rxn} for the reaction is -1052.8 kJ.

7 0
3 years ago
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