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Black_prince [1.1K]

3 years ago

14

Suppose that magnesium would react exactly the same as copper in this experiment. how many grams of magnesium would have been us

ed in the reaction if 1.000 g of silver were produced? the atomic mass of magnesium is 24.31 g/mol, and the atomic mass of silver is 107.87 g/mol

1 answer:

Vikentia [17]3 years ago

6 0

The solution for this problem would be:

We are looking for the grams of magnesium that would have been used in the reaction if one gram of silver were created. The computation would be:

1 g Ag (1 mol Mg) (24.31 g/mol) / (2mol Ag)(107.87g/mol) = 0.1127 grams of Magnesium

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A 21.8 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature ris

Blababa [14]

<u>Answer:</u> The heat capacity of calorimeter is $15.66J/^oC$

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Given mass of ethanol = 21.8 g

Molar mass of ethanol = 46.07 g/mol

Putting values in above equation, we get:

$\text{Moles of ethanol}=\frac{21.8g}{46.07g/mol}=0.473mol$

To calculate the enthalpy change of the reaction, we use the equation:

$\Delta H_{rxn}=\frac{q}{n}$

where,

$q$ = amount of heat released = ?

n = number of moles = 0.473 moles

$\Delta H_{rxn}$ = enthalpy change of the reaction = -1235 kJ/mol = $-1235\times 10^3J/mol$ (Conversion factor: 1 kJ = 1000 J)

Putting values in above equation, we get:

$-1235\times 10^3J/mol=\frac{q}{0.473mol}\\\\q=(-1235\times 10^3J/mol\times 0.473mol)=-584.16\times 10^3J$

To calculate the heat capacity of calorimeter, we use the equation:

$q=c\Delta T$

where,

q = heat absorbed by the calorimeter = $584.16\times 10^3J$

c = heat capacity = ?

$\Delta T$ = change in temperature = $T_2-T_1=62.3^oC-25^oC=37.3^oC$

Putting values in above equation, we get:

$584.16\times 10^3J=c\times 37.3^oC\\\\c=\frac{584.16\times 10^3J}{37.3^oC}=15.66J/^oC$

Hence, the heat capacity of calorimeter is $15.66J/^oC$

4 0

4 years ago

What isotope is formed when u-238 emits an alpha particle?.

yarga [219]

A nucleus of uranium 238 decays by alpha emission to form a daughter nucleus, thorium 234.

<h3>What are isotopes?</h3>

Isotopes are atoms with the same number of protons but differ in numbers of neutrons.

Uranium-238 produces thorium-234 by alpha decay.

An α-particle is a helium nucleus. It contains 2 protons and 2 neutrons, for a mass number of 4.

During α-decay, an atomic nucleus emits an alpha particle. It transforms (or decays) into an atom with an atomic number 2 less and a mass number 4 less.

Thus, uranium-238 decays through α-particle emission to form thorium-234 according to the equation:

$^{238}_{92}U\;\rightarrow\;^{234}_{90}Th\;+\;^4_2He$

Learn more about the isotopes here:

brainly.com/question/11680817

#SPJ1

4 0

2 years ago

Given thatH2(g) + F2(g) -> 2HF(g) => ∆H = -546.6 kJ . mol-12H2(g) + O2(g) -> 2H20(l) => ∆H = -571.6 kJ. mol-1

Fantom [35]

<u>Answer:</u> The $\Delta H^o_{rxn}$ for the reaction is -521.6 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 chemical equation for the reaction of fluorine and water follows:

$2F_2(g)+2H_2O(l)\rightarrow 4HF(g)+O_2(g)$ $\Delta H^o_{rxn}=?$

The intermediate balanced chemical reaction are:

(1) $H_2(g)+F_2(g)\rightarrow 2HF(g)$ $\Delta H_1=-546.6kJ$ ( × 2)

(2) $H_2(g)+O_2(g)\rightarrow 2H_2O(g)$ $\Delta H_2=-571.6kJ$

The expression for enthalpy of reaction follows:

$\Delta H^o_{rxn}=[2\times \Delta H_1]+[1\times (-\Delta H_2)]$

Putting values in above equation, we get:

$\Delta H^o_{rxn}=[(2\times (-546.6))+(1\times (571.6))]=-521.6kJ$

Hence, the $\Delta H^o_{rxn}$ for the reaction is -521.6 kJ.

8 0

3 years ago

John (travel) to Russia next week correct the tense

kondor19780726 [428]

Answer:

hi

Explanation:

John will travel to Russia next week

hope it helps

have a nice day

7 0

3 years ago

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The substances on the left side of a chemical equation are called the:

torisob [31]

B compnests is the answe tot his quotation

8 0

2 years ago