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kogti [31]
3 years ago
12

A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are

Chemistry
1 answer:
Butoxors [25]3 years ago
7 0
<h3>Answer:</h3>

82.11%

<h3>Explanation:</h3>

We are given;

  • Theoretical mass of the product is 137.5 g
  • Actual mass of the product is 112.9 g

We are supposed to calculate the percentage yield

  • We need to know how percentage yield is calculated;
  • To calculate the percentage yield we get the ratio of the actual mass to theoretical mass and express it as a percentage.

Thus;

% yield = (Actual mass ÷ Experimental mass) × 100%

            = (112.9 g ÷ 137.5 g) × 100%

            = 82.11%

Therefore, the percentage yield of the product is 82.11 %

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5F248+ 2NH3(8) ► NF418 + 6HF
mylen [45]

Answer:

14.2L at STP

Explanation:

Based on the problem, 2 moles of NH3 produce 6 moles of HF. To solve this question we have to convert the mass of NH3 to moles. With the chemical equation find the moles of HF and using PV = nRT find the liters of HF:

<em>Moles NH3 -Molar mass: 17.031g/mol-</em>

3.6g NH3 * (1mol / 17.031g) = 0.211 moles NH3

<em>Moles HF:</em>

0.211 moles NH3 * (6mol HF / 2mol NH3) = 0.634 moles HF

<em>Volume HF</em>

PV = nRT; V = nRT/P

<em>Where V is volume in liters, n are moles of the gas = 0.634 moles, R is gas constant = 0.082atmL/molK, T is absolute temperature = 273.15K at STP and P is pressure = 1atm at STP.</em>

Replacing:

V = 0.634moles*0.082atmL/molK*273.15K / 1atm

V = 14.2L at STP

6 0
2 years ago
Calculate [OH−] for each solution.
Triss [41]

Answer:

1.  [OH⁻] = 0.30 M ; 2. [OH⁻] = 1.54x10⁻⁶M ; 3. [OH⁻] = 1.32x10⁻¹³M

Explanation:

Remember the rule:

pH + pOH = 14

pOH = 14 - pH

10*⁻pOH (you have to elevate 10, to -pOH)

10*⁻pOH  = [OH⁻]

1. 14 - 13.48 = 0.52

10⁻⁰°⁵² = 0.30

2. 14 - 8.19 = 5.81

10⁻⁵°⁸¹ = 1.54x10⁻⁶

3. 14 - 2.12 = 12.88

10⁻¹²°⁸⁸ = 1.32x10⁻¹³

6 0
3 years ago
Two atoms that are isotopes of one another must have the same number of what?
erastovalidia [21]
They must have the same number of protons
6 0
2 years ago
Read 2 more answers
Carry out the following calculation, paying special attention to the significant figures (where 4/3 is exact), rounding, and uni
babunello [35]

Answer:

Value = 1.80 g/cm³ (Approx)

Explanation:

Given:

\frac{3.39 \times 10^7g}{(\frac{4}{3} )(3.1416)(1.65 \times 10^2 cm)^3}

Computation:

\frac{3.39 \times 10^7g}{(\frac{4}{3} )(3.1416)(1.65 \times 10^2 cm)^3} \\\\\frac{3.39 \times 10^7g}{(\frac{4}{3} )(3.1416)(4.492125 \times 10^6 cm^3)} \\\\ \frac{3.39 \times 10^7g}{(\frac{4}{3} )(3.1416)(4.492125 \times 10^6 cm^3)}\\\\ \frac{3.39 \times 10^7g}{18.8166132\times 10^6 cm^3} \\\\ 1.80159945g/cm^3

Value = 1.80 g/cm³ (Approx)

7 0
3 years ago
If equal volumes of 0.1 M HCl and 0.2 M TRIS (base form) are mixed together. The pKa of TRIS is 8.30. Which of the following sta
blondinia [14]

Answer:

option D is correct

D. This solution is a good buffer.

Explanation:

TRIS (HOCH_{2})_{3}CNH_{2}

if TRIS is react with HCL it will form salt

(HOCH_{2})_{3}CNH_{2} + HCL ⇆   (HOCH_{2})_{3}NH_{3}CL

Let the reference volume is 100

Mole of TRIS is =  100 × 0.2 = 20

Mole of HCL is =  100 × 0.1 = 10

In the reaction all of the HCL will Consumed,10 moles of the salt will form

and 10 mole of TRIS will left

hence , Final product will be salt +TRIS(9 base)

H = Pk_{a} + log (base/ acid)

8.3 + log(10/10)

8.3

6 0
3 years ago
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