There are 3 significant figures in 0.0000246 g.
The product of 0.12 g, 1.8 g, and 0.562 g should have the same number of significant figures as the measurement with the fewest significant figures, which is 0.12 g in this case. Therefore, the product should be expressed with two significant figures.
143 g has three significant figures. The leading zeros are not considered significant.
it would be 0.03 just round up, two significant figures means two figures after the decimal point. If it was 3 significant figures then it would be 0.04 etc....
1 mole H2O = 18.02g --- water is H2O ... 2 x 1.008 + 1 x 15.996 = 18.012 g/mole = 18.01 grams
To find the number of moles in 1.18 g of NO2, you need to divide the given mass by the molar mass of NO2. The molar mass of NO2 is approximately 46 g/mol. So, 1.18 g / 46 g/mol = roughly 0.026 moles of NO2.
There are 2 significant figures in this measurement.
The product of 0.12 g, 1.8 g, and 0.562 g should have the same number of significant figures as the measurement with the fewest significant figures, which is 0.12 g in this case. Therefore, the product should be expressed with two significant figures.
2 significant figures.
2 significant figures.
143 g has three significant figures. The leading zeros are not considered significant.
2 of them.
6 of them.
5
4 of them.
5 of them.
There are two significant figures.
Three.