Compounds A and B are colorless gases obtained by combining sulfur with oxygen. Compound A results from combining 6.00 g of sulfur with 5.99 g of oxygen, and compound B results from combining 8.60 g of sulfur with 12.88 g of oxygen. Show that the mass ratios in the two compounds are simple multiples of each other.

1.5

Explanation:

Given that :

Compound A and B are formed from Sulfur + Oxygen.

Compound A :

6g sulfur + 5.99g Oxygen

Compound B:

8.6g sulfur + 12.88g oxygen

Comparing the ratios :

Compound A:

S : O = 6.00 : 5.99

S/0 = 6.0g S / 5.99g O

Compound B :

S : O = 8.60 : 12.88

S / O = 8.60g S / 12.88g O

Mass Ratio of A / mass Ratio of B

(6.0g S / 5.99g O) ÷ (8.60g S / 12.88g O)

(6.0 g S / 5.99g O) × (12.88g O / 8.60g S)

(6 × 12.88) / (5.99 × 8.60)

= 77.28 / 51.514

= 1.50017

= 1.5

52.17%

Explanation:

Number of matches in the box = 46

Number of matches that lit on the first strike = 22

Number of matches that did not light on the first strike = 46 - 22 = 24

Therefore, the percentage of the matches in the box did not light on the first strike will be:

= (Number of matches that did not light on the first strike / Number of matches in the box) × 100

= 24/46 × 100

= 52.17%

Therefore, the percentage of the matches in the box that did not light on the first strike is 52.17%.