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64 gram methane are mixed with 64 gram of oxygen and burnt,then the mass of carbondioxide obtained is?
The Stoichiometric equation for the reaction is CH4 + 2O2 = CO2 + 2H2OMoles of CH4 = 64/16 = 4Moles of O2 = 64/32 = 2For every 2 moles of...
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Differentiate between bulk sample, primary sample, secondary sample, subsample, laboratory sample, and test sample.
A bulk sample is the physical sample of a large volume or tonnage of mineral material taken from a known resource area for investigative purposes.Primary sampling unit refers to Sampling...
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A chemist needs 2.38 grams of a liquid compound with a density of 0.718 g/cm3. What volume of the compound is required?
V = m/d = 2.38g/(0.718g/cm3) = 3.315 cm3
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weight of 1 atom of an element is 6.644 into 10 power -23 gram .Calculate gram atom of element in 40 kg
We must know how many atoms is in 40 kg. N = 40000 g / 6.644 * 10^ -23 = 6020 * 10^23 atoms gramatom is 6020*10^23 / 6.02*10^23 =...
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What mass of ethanol is needed to create 2.5 gram of ethanoic acid (CH3COOH)? assume the ratio of ethanol to ethanoic acid needed is 1:1
m(CH3CH2OH) = 2,5g n(CH3CH2OH) : n(CH3COOH) = 1: 1 m(CH3COOH) = ? X g 2.5g CH3CH2OH → CH3COOH 46 g/moll 60 g/moll 46g (CH3CH2OH) ─ 60g (CH3COOH) X g (CH3CH2OH)...
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A 30.84 mL sample of 0.128 M NaOH is needed to reach an endpoint for a titration of a 5.441 gram sample of Vinegar. Calculate the % acetic acid in the vinegar sample. (Show all work)
First calculate the moles of acetic acid, then the weight of acetic acid, then divide by the weight of vinegar. 1. moles of acetic acid is equivalent to moles of...
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An unknown liquid was found to have a density of 69.22lb/ft3. The density of ethylene glycol (the liquid used in antifreeze)is 1.1088 g/mL. Is the unknown liquid ethylene glycol?
69.22lb/ft3=1.1088 g/mL.Therefore the unknown liquid is ethylene glycol.
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112 mL of NO2(g) at STP was liquefied, the density of the liquid being 1.15 g mL
Calculate the volume of liquid and the number of molecules in the liquid NO2
One mole of an ideal gas will occupy a volume of 22.4 liters at STP (Standard Temperature and Pressure, 0°C and one atmosphere pressure).Proportion:1 mole – 22400 mln moles –...
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The liquid 1-iodobutane has a density of 1.62 g/mL at 20.0 °C. If a 143 gram sample of this compound is needed, what volume of the liquid at 20.0 °C must be provided? volume=...............ml
Volume = Mass / Density = 143g / 1.62g/mL = 88.27mL
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The liquid iodobenzene has a density of 1.83 g/mL at 20.0 °C. If a 56.4 mL sample of this compound is provided, what is the mass of the liquid at 20.0 °C that must be provided? Mass=...........g
density = mass/volume density = 1.83g/ml , volume = 56.4ml at 20⁰Cmass = density×volume mass = 1.83×56.4 mass = 103.2 g
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