# chemistry

3. Use the mole ratio of CuO produced per mole of malachite to write a balanced equation for the malachite decomposition reaction. Assume that CO₂ is also a product of the decomposition.

CuCo3*Cu9OH)2 -----> 2Cuo+Co2+H2O

0.004522431 moles of malachite
0.01257071 moles of CuO

4. Predict the mass of CuO expected to result from the decomposition of the malachite, based on the balanced equation. 1g of Malachite was given. The mass of CuO produced (g): 0.72g

5. Compare the mass obtained from the mass predicted, and discuss reasons for any discrepancy.

1. 👍
2. 👎
3. 👁
1. It appears t me that 0.00452 moles malachite should have produced 2x that for CuO. Is that 0.0126 mols your experimental value? If so it is too high. I have no idea what may have gone wrong. You have provided no details for the experiment.

1. 👍
2. 👎
2. (a) Mass of an empty Erlenmeyer flask (g): 91.780g

(b) Mass of the Erlenmeyer flask with malachite(g): 92.780g

(c) Subtract (a) from (b) to obtain the mass of malachite (g): 1g

(c) Mass of Erlenmeyer flask with CuO(g): 92.500g

(d) Subtract (a) from (c) to obtain the mass of CuO produced (g): 0.72g

2. Calculate the following:

(a) moles of malachite in 1g: 222.1mw
0.004522431 moles of malachite

(b) moles of CuO produced: 79.55 mw

0.01257071 moles of CuO

1. 👍
2. 👎
3. If I read this right,
moles malachite in 1 g i 1/221.12 = 0.0452 (we have a slight difference in molar mass malachite--based on CuCO3.Cu(OH)2 I found 221.12) but that changes your value insignificantly.

Next. 0.72 looks ok BUT moles from that does not. If I divide 0.72/79.55 I get 0.00905 and not the 0.0126 you have.

Based on the 0.00452 moles of malachite you took you should have obtained 0.00452 x 2 = 0.00904 and that is just about as good as it gets in lab work.You don't have an error to explain. :-).

1. 👍
2. 👎

## Similar Questions

1. ### Chemistry

A solution of I2 was standardized with ascorbic acid. Using a 0.1000-g sample of pure ascorbic acid (C6H8C6), 25.32 ml of I2 were required to reach the starch end point. What is the molarity of the iodine solution? Please check to

2. ### chemistry

given the reactant amounts specified in each chemical eguation, determine the limiting reactant in each case: a. HCL+NaOH->NaCl+H2O 2.0 mole of HCl 2.5 mole NaOH b. Zn+2HCl->ZnCl2+H2 2.5 mole Zn 6.o mole HCl c.

3. ### Chemistry

Billions of pounds of urea are produced annually for use as a fertilizer The reaction used is 2NH3+CO2=CO(NH2)2+H2O The typical starting mixture has 3:1 mole ratio of NH3 to CO2 .If 47.7grams urea form per mole of CO2 that reacts

4. ### chemistry

One M&M candy has a volume of 1.0mL. What volume, in cubic meters, would one mole of M&M candies occupy? 2) For this next calculation, you’re going to compare the volume of a mole of M&Ms to Lake Erie, which has a volume of

1. ### CHEM

a mixture of 10cm3 of methane and 10cm3 of enthane was sparked with an excess of oxygen. after coolin to room temp, the residual gas was passed through aq KOH. what volume of gas was absorbed by the alkali ? Write the equations

2. ### CHEMISTRY

Which of the following solutions contain the greatest total ion concentration? a) one mole of potassium chloride dissolved in 1.0L of solution b)one mole of sodium phosphate dissolved in 1.0L of solution c)one mole of ammonium

3. ### CHEM HELP

what is the theoretical mole ratio- NaCl to NaHCO3 How do you determine the percentage error of an experimental mole ratio It would be easier for us to help you if we had the entire problem instead of just parts of it. However,

4. ### chemistry

Determine the theoretical yield of C when each of the following amounts of A and B are allowed to react in the generic reaction: A+2B-->3C 1) 1mol A; 1 mole B 2) 1mole A; 3 mole B 3) 2mole A; 2 mole B 4) 32mole A; 68 mole B

1. ### chemistry

2.2. Billions of kilograms of urea, are produced annually for use as a fertilizer. The reaction used is given below. NH3(g) + CO2(g) → CO(NH2)2(s) + H2O(l) The typical starting reaction mixture has a 3:1 mole ratio of NH3 to

2. ### Chemistry (Thermodynamics)

Write a balanced equation for the complete combustion of 1 mole of ethyne gas (C2H2) ?

3. ### Chemistry

What volume of 3.0M Na2SO4 must be added to 25ml of 1.0M BaCl2 to produce 5.0g of BaSO4? The answer is 7.1ml but I don't get it very well. I thought I could use mole ratio of the balanced equation, but it did not work. Thanks a

4. ### Chemistry

Determine the simplest formula for compounds that have the following analyses. The data may not be exact. A. 28.5% iron, 48.6% O, 22.9% S This is what I did: 28.5g Fe 1 mole Fe/55.847g = .51 mole 48.6g O 1 mole O/15.999g = 3.04