Chemistry, 20.10.2019 22:00 mremoney530

In the reaction below, how many grams of h2o(g) are produced when 2.1 grams o2(g) are consumed? c4h6(g) + o2(g) → co2(g) + h2o(g)
a. 1.2
b. 660
c. 0.64
d. 2.2
e. 0.0020

Answers: 3

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Answer from: aschool2000

0.64 grams of H₂O

Further explanation

Given:

The combustion reaction of C₄H₆ consumes 2.1 grams of oxygen gas.

Question:

How many grams of H₂O is produced?

The Process:

Step-1

Relative atomic mass: O = 16, and H = 1.Relative molecular mass (Mr) of O₂ = 2 x 16 = 32.Relative molecular mass (Mr) of H₂O = 2(1) + 16 = 18.

Let us convert mass to mol of 2.1 g of O₂.

$\boxed{ \ n = \frac{mass}{Mr} \ } \rightarrow \boxed{ \ n = \frac{2.1}{32} = 0.0656 \ moles \ }$

Therefore, 0.0656 moles of O₂ are consumed.

Step-2

Balanced reaction:

$\boxed{ \ 2C_4H_6_{(g)} + 11O_2_{(g)} \rightarrow 8CO_2_{(g)} + 6H_2O_{(g)} \ }$

Due to excess C₄H₆, then O₂ become the limiting reagent. The number of moles of O₂ determines the number of moles of H₂O as a result.

According to the chemical equation above, the proportion between O₂ and H₂O is 11 to 6. Therefore, we can count the number of moles of H₂O.

$\boxed{ \ \frac{n(H_2O)}{n(O_2)} = \frac{6}{11} \ }$ $\ \rightarrow \boxed{ \ n(H_2O) = \frac{6}{11} \times n(O_2) \ }$

$\boxed{ \ n(H_2O) = \frac{6}{11} \times 0.0656 \ }$

n (H₂O) = 0.0358 (round off to four decimal places)

Hence we get 0.0358 moles of H₂O.

Step-3

Let us convert mol to mass of 0.12 moles of H₂O.

$\boxed{ \ n = \frac{mass}{Mr} \ } \rightarrow \boxed{ \ mass = n \times Mr \ }$

$\boxed{ \ mass = 0.0358 \ moles \times 18 \ \frac{g}{mol} \ }$

$\boxed{ \ mass = 0.64 \ grams \ }$ (round off to two decimal place)

Thus, we can produce 0.64 grams of H₂O.

Learn moreHow many grams of Ca(NO₃)₂ can be produced? Determine the mass of aspirin from the number of molecules How many molecules are in 43.5 g a sample of ammonia? How many grams of sodium hydroxide are needed to make 250 ml of a 7.80 M solution?

Answer from: Quest

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is $1s^{2}2s^{2}2p^{6}3s^{1}$ and electronic configuration of phosphorous is $1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}$ .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

$3na + p \rightarrow na_{3}p$

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

Electrons are transferred from atoms of to atoms of this transfer makes the sodium atoms and the

Answer from: Quest

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