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luda_lava [24]
3 years ago
5

A student goes into a lab and performs an experiment which produces 4.56grams

Chemistry
1 answer:
Murrr4er [49]3 years ago
6 0

Answer:

can you help me with my chemistry?

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One way to measure temperature in some applications is to monitor the gas pressure in a rigid, closed container. What is the tem
julia-pushkina [17]

Answer:

296.43 K is the temperature of a vessel when pressure reads 1.250 atm.

Explanation:

At STP, when pressure is 1.000 atm the value of temperature is 273,15 K.

If the pressure at temperature T reads as 1.250 atm.

P_1=1.000 atm, T_1=298.15K

P_2=1.250 atm,T_2=?

Applying Gay Lussac's law:

\frac{P_1}{T_1}=\frac{P_2}{T_2} (At constant volume)

\frac{1.000 atm}{273.15 K}=\frac{1.250 atm}{T_2}

T_2=296.43 K

296.43 K is the temperature of a vessel when pressure reads 1.250 atm.

6 0
3 years ago
HELP! PLEASE! ASAP! Manganese(III) fluoride, MnF3, can be prepared by the following reaction:
Crank

Answer:

14.336 g MnF₂

Explanation:

number of moles = mass / molecular weight

number of moles of MnI₂ = 55 / 309 = 0.178 moles

number of moles of F₂ = 55 / 38 = 1.447 moles

From the reaction and the number of moles calculated we deduce that the fluorine F₂ is a limiting reactant.

So:

if        13 moles of F₂ reacts to produce 2 moles of MnF₃

then   1.447 moles of F₂ reacts to produce X moles of MnF₃

X = (1.447 × 2) / 13 = 0.223 moles of MnF₃ (100% yield)

For 57.2% yield we have:

number of moles of MnF₃ = (57.2 / 100) × 0.223 = 0.128 moles

mass = number of moles × molecular weight

mass of MnF₃ = 0.128 × 112 = 14.336 g

3 0
3 years ago
Calculate the mass (in grams) of calcium carbonate present in a 50.00 mL sample of an aqueous calcium carbonate standard, assumi
horrorfan [7]
1 part per million is the same as 

<span>1 mcg/mL (mcg = 1 micro gram = 1 * 10^-6 grams). </span>
<span>125 ppm = 125 mcg/mL </span>

<span>125 mcg/ml * [1 gram / 1 * 10^6 mgrm] = 1.25 * 10^-4 grams </span>

<span>The density of hard water is 1.000 grams / mL </span>

<span>50 mL of water contains 1.25 * 10^-4 grams. </span>

<span>given mass = 1.25 * 10^-4 </span>
<span>Molar mass = 100.0 grams / mole </span>
<span>n = ????? </span>

<span>n = 1.25 * 10^-4/100 = 1.25 * 10^-6 moles. 

Thank you for posting your question here at brainly. I hope the answer will help you. Feel free to ask more questions.

</span>
7 0
3 years ago
The entropy of a system at 337 K increases by 221.7 J/mol•K. The free energy value is found to be –717.5 kJ/mol. Calculate the c
OlgaM077 [116]

<u>Answer:</u> The change in enthalpy for the given system is -642.8 kJ/mol

<u>Explanation:</u>

To calculate the change in enthalpy for given Gibbs free energy, we use the equation:

\Delta G=\Delta H-T\Delta S

where,

\Delta G = Gibbs free energy = -717.5 kJ/mol = -717500 J/mol    (Conversion factor: 1 kJ = 1000 J)

\Delta H = change in enthalpy = ?

T = temperature = 337 K

\Delta S = change in entropy = 221.7 J/mol.K

Putting values in above equation, we get:

-717500J/mol=\Delta H-(337K\times 221.7J/mol.K)\\\\\Delta H=-642787J/mol=-642.8kJ/mol

Hence, the change in enthalpy for the given system is -642.8 kJ/mol

4 0
4 years ago
Which is a pure substance?
Ad libitum [116K]
Pure substances are made of the same material and have almost the same properties such as: Carbon, Iorn, Water, Sugar, Salt, and Nitrogen.
8 0
3 years ago
Read 2 more answers
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