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

0.64 grams of H₂O

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

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

Therefore, 0.0656 moles of O₂ are consumed.

Step-2

Balanced reaction:

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.

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.

(round off to two decimal place)

Thus, we can produce 0.64 grams of H₂O.

the electrical  conductivity  of asolution  of an electrolyte is measured by determining the resistance of thesolution  between two flat or cylindrical electrodes separated by a fixed distance.

i would say b

explanation:

but i think i would need more information than that