Radius of the metallic ball, r = \(\frac{4.2}{2}\) cm = 2.1cm
The volume of the metallic ball = \(\frac{4}{3}\pi r^3 \)
= \(\frac{4}{3}\) × \(\frac{22}{7}\) × 2.1cm × 2.1cm × 2.1cm
= 38.808 cm³
Mass = Volume × Density
Mass of the metallic ball = 38.808 cm3 × 8.9g / cm³
= 345.3912 g
= 345.39 g
Hence, the mass of the ball is 345.39 g (approximately).
When 3.0g of carbon is burnt in 8.00g oxygen, 11.00g of carbon dioxide is produced. What mass of carbon dioxide will be formed when 3.00g of carbon is burnt in 50.0g of oxygen? Which law of chemical combination will govern your answer?