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Andrew [12]
3 years ago
5

determine the type of the following chemical reaction: Mg(s) + 2HCl(aq)——-> H2(g) + MgCl2(aq) a. single replacement reaction

b. decomposition reaction c. combination reaction d. double replacement reaction
Chemistry
1 answer:
kumpel [21]3 years ago
4 0

Answer:

a. single replacement reaction

Explanation:

Mg(s) + 2HCl(aq)——-> H2(g) + MgCl2(aq)

Mg replaces H, so this is a single replacement reaction.

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A gold-colored ring has a mass of 17.5 grams and a volume of 0.82 mL. What is the density of this ring?
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Answer:

21 g/mL

Explanation:

To solve this problem, first look at the density equation, which is D=M/V, which D stands for density, M stands for mass, and V stands for volume. When you substitute in the variables, you get D=17.5/.82, which is equivalent to 21.34. However, since we need to pay attention to the sig fig rules for multiplying, we need to have the same amount of sig figs as the value with the least amount of sig figs, which is the number .82. .82 has two sig figs, so you round down. Your answer will be 21 g/mL.

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3 years ago
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Answer:

1.) 3

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Explanation:

1. Density=\frac{MASS}{VOLUME}= \frac{75}{25}

2. Length*Width*Height=3*10*2

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3 years ago
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3 years ago
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Answer:

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2 years ago
What temperature will the water reach when 10.1 g CaO is dropped into a coffee cup containing 157 g H2O at 18.0°C if the followi
Zepler [3.9K]

Answer:

Final temperature attained by water = 34.6°C

Explanation:

The reaction of CaO and H₂O is an <em>exothermic reaction</em>. The equation of reaction is given below:

CaO + H₂O ----> Ca(OH)₂

The quantity of heat given off, ΔH°rxn = 64.8KJ/mol = 64800J/mol

Number of moles of CaO = mass/molar mass, where molar mass of Ca0 = 56g/mol, mass of CaO = 10.1g

Number of moles of CaO = 10.1g/56g/mol =0.179moles

Quantity of heat given off by 0.179 moles = 64800 *0.179 = 11599.2J/mol

Using the formula, <em>Quantity of heat, q = mass * specific heat capacity * temperature rise.</em>

mass of mixture = (10.1 + 157)g = 167.1g, Initial temperature = 18.0°C

Final temperature(T₂) - Initial temperature(T₁) = Temperature rise

11599.2J/mol = 167.1g * 4.18J/g·°C * ( T₂ - 18.0°C)

11599.2 = 698.478T₂ - 12572.604

11599.2 + 12572.604 = 698.478T₂

698.478T₂ = 24171.804

T₂ = 34.6°C

Therefore, final temperature attained by water = 34.6°C

6 0
3 years ago
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