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Question 4What is the sum of these two reactions? Write your answer below, but don't worry about formatting with subscripts-Do write chemical formulas with
proper atomic symbols, though (e.g., write CuCl2, not CUCL2).
(1) Ca + 2HCl - CaCl2 + H2
(2) CaCl2+H2O = CaO + 2HCl

Answers

Answer 1

Answer:

Answer:

$Ca +H_2O \rightarrow + H_2 + CaO$

Explanation:

Hello,

In this case, considering the given two reactions, when we add them, we obtain:

$Ca + 2HCl +CaCl_2 +H_2O \rightarrow CaCl_2 + H_2 + CaO+2HCl$

Thus, we can simplify both hydrochloric acid and calcium chloride as they are both sides to obtain:

$Ca +H_2O \rightarrow H_2 + CaO$

Best regards.

Related Questions

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A volume of 40.0 mLmL of aqueous potassium hydroxide (KOHKOH) was titrated against a standard solution of sulfuric acid (H2SO4H2SO4). What was the molarity of the KOHKOH solution if 16.2 mLmL of 1.50 MM H2SO4H2SO4 was needed? The equation is 2KOH(aq)+H2SO4(aq)→K2SO4(aq)+2H2O(l)
Assuming binding is fast relative to subsequent catalytic steps, what relative effect does substitute the various active site residues have on catalysis versus substrate-binding? The various substitutions affecta. substrate-binding more than catalytic turnover. b. catalytic turnover more than substrate binding. c. substrate binding, but not catalytic turnover. d. catalytic turnover, but not substrate binding.
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All light travels at the same speed.O TrueO False

A structural model of retinol is shown below. How many carbon atoms are inretinol?
А. 14
В. 28
С. 20
D. 5

Answers

Answer:

The answer is 20

Explanation:

What is the molecular formula of each of the following compounds? Part A Empirical formula CHO2, molar mass = 180.0 g/mol

Answers

Answer:

C4H4O8

Explanation:

The molecular formula of a compound with empirical formula: CHO2 can be calculated as follows:

(CHO2)n = 180g/mol

{12 + 1 + 16(2)}n = 180

(12+1+32)n = 180

(45)n = 180

n = 180/45

n = 4.

The molecular formula = (CHO2)4

= C4H4O8

How many significant digits are in 89015?

Answers

Answer:5

Explanation:

Cobalt chloride Select one: a. Forms a single hydrate which may be pink or blue
b. Is colorless in the presence of water
c. Does not exist as a hydrate
d. Forms different hydrates which have different colors

Answers

Answer:Forms different hydrates which have different colors

Explanation:

CoCl2 in its anhydrous form is blue in colour. This anhydrous compound could absorb moisture, first forming the purple dihydrate and absorbs more water molecules to form the hexahydrate. Hence various hydrates of cobalt II chloride have different colours as stated above. Equations of reaction for the formation of the two hydrates are attached.

A student is given a sample of a blue copper sulfate hydrate. He weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. The mass of the empty crucible and lid was found earlier to be 22.652 g. He then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. On colling, he finds the mass of crucible, lid, and contents to be 23.403 g. The sample was changed in the process to very light clue anhydrous CuSO4. How many moles of water are present per mole of CuSO4?

Answers

Answer:

There are present 5,5668 moles of water per mole of CuSO₄.

Explanation:

The mass of CuSO₄ anhydrous is:

23,403g - 22,652g = 0,751g.

mass of crucible+lid+CuSO₄ - mass of crucible+lid

As molar mass of CuSO₄ is 159,609g/mol. The moles are:

0,751g × $(1mol)/(159,609g)$ = 4,7052x10⁻³ moles CuSO₄

Now, the mass of water present in the initial sample is:

23,875g - 0,751g - 22,652g = 0,472g.

mass of crucible+lid+CuSO₄hydrate - CuSO₄ - mass of crucible+lid

As molar mass of H₂O is 18,02g/mol. The moles are:

0,472g × $(1mol)/(18,02g)$ = 2,6193x10⁻² moles H₂O

The ratio of moles H₂O:CuSO₄ is:

2,6193x10⁻² moles H₂O / 4,7052x10⁻³ moles CuSO₄ = 5,5668

That means that you have 5,5668 moles of water per mole of CuSO₄.

I hope it helps!

Consider the following reaction: 2NO(g)+O2(g)→2NO2(g) Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.) 718k

Answers

Final answer:

The Gibbs free energy change (ΔG∘) for the reaction can be estimated using the equation ΔG∘ = ΔH∘ - TΔS∘. At a temperature of 718K, if ΔG∘ is negative, the reaction will be spontaneous.

Explanation:

The Gibbs free energy change (ΔG∘) for a reaction can be estimated using the equation ΔG∘ = ΔH∘ - TΔS∘, where ΔH∘ is the change in enthalpy and ΔS∘ is the change in entropy. At a temperature of 718K, you can estimate ΔG∘ by substituting the given values into the equation. If the value of ΔG∘ is negative, the reaction will be spontaneous. If it is positive or zero, the reaction will not be spontaneous.