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The synthesis portion of photosynthesis is sometimes referred to as fixation; that is, the gas $CO_2$ is "fixed" into an organic molecule. Of the four major types of organic molecules, into which is $CO_2$ first fixed?
$CO_2$ taken in by the plant initially bonds to ribulose 1,5-biphosphate or $RuBP$ to form an unstable 6-carbon compound. This then divides into two three-carbon of glycerate 3-phosphate. With the...
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Given this reaction: $CH_4 + 2O_2 -> CO_2 + H_2O$, 16 g of $CH_4$ react with 64 g of $O_2$, producing 44 g of $CO_2$. How many grams of water are produced?
There are actually two methods of doing it - stoichimetry & also with the help of law of conservation of mass. First by : $16$grams of $CH_4$ means $1$mole of...
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How many molecules of $CO_2$ are there in 55 grams of $CO_2$?
By definition there are $6.022xx10^23$ carbon dioxide molecules in a $44.0*g$ mass. How do I know this? Well because we use the given number to specify molar mass, the which...
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$39 x 10^22$ molecules of $CO_2$ is equal to how many moles of $CO_2$?
You have $3.90xx10^23$ molecules, and the molar quantity is the simply the quotient, $(3.90xx10^23*"molecules")/(6.022xx10^23*"molecules"*mol^-1)$ $=$ $??mol$
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For $CH_4 +2O_2 -> CO_2 + 2H_2O$, the molar mass of oxygen gas ($0_2$) is 32.00 g/mol. The molar mass of carbon dioxide ($CO_2$) is 44.01 g/mol. What mass of $CO_2$, in grams, will form when 8.94 g $O_2$ completely react?
The balanced chemical equation tells us unequivocally that 16 g of methane gas reacts with 32 g of dioxygen gas to give 44 g of carbon dioxide, and 36 g...
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How many grams of $CO_2$ are produced from 125 g of $O_2$ and excess $CH_4$ in the equation $CH_4 +2O_2-> CO_2 + 2H_2O$?
Here $CH_4$ being excess $O_2 $ will be consumed fully. We know from above equation 2 mole or 64 g $O_2$ produces 1 mole or 44 g $CO_2$ So 125...
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For the reaction,$2x$+$3y$+$4z$$ rarr$$ 5w$
Initially if 1 mole of $x$,3 mole of $y$ and 4 mole of $z$ is taken and 1.25 mole of $w$ is obtained then what is the % yield of this reaction?
This is a limiting reactant problem. We know that we will need a balanced equation and moles of each reactant. 1. Gather all the information in one place with...
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$CO_2$ gas, in the dry state, may be produced by heating calcium carbonate. $CaCO_3 (s)DeltaCaO(s) + CO_2(g)$. What volume of $CO_2$, collected dry at 55 C and a pressure of 774 torr, is produced by complete thermal decomposition of 10.0 g of $CaCO_3$?
$10gramsCaCO_3(s) => CaO(s) + (?)O_2(g)$ $"moles" CaCO_3 = ((10g)/(100(g/(mol))))$ = $0.10"mole"$ From reaction ratios => moles $CaCO_3(s)$ consumed = moles $O_2(g)$ produced = 0.10 mole $(O_2(g))$**** If a 'dry'...
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The concentration of $CO_2$ in a can of soda is approximately 0.045 M. If all of the $CO_2$ in a 12 ounce soda evolves from solution, how many liters would the $CO_2$ gas take up at STP?
The idea here is that you need to figure out how many moles of carbon dioxide, $"CO"_2$, are initially dissolved in the soda by using the volume and of...
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Which sample has the most number of atoms?
$A.$ $"1 mole of oxygen atoms;"$
$B.$ $"1 mole of oxygen molecules;"$
$C.$ $"1 mole of ozone molecules;"$
$D.$ $"Each sample contains the same number of atoms."$
Mass is a measure of the number of particles. Here you have $O$ atoms, and dioxygen, $O_2$, and ozone molecules, $O_3$ but each have the same mass by specification. There...
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